Semiconductor-based Photocatalytic Hydrogen Generation - American

Chem. Rev. 2010, 110, 6503–6570

6503

Semiconductor-based Photocatalytic Hydrogen Generation Xiaobo Chen,*,† Shaohua Shen,†,‡ Liejin Guo,‡ and Samuel S. Mao† Lawrence Berkeley National Laboratory, Berkeley, California 94720, United States, and State Key Laboratory of Multiphase Flow in Power Engineering, Xi’an Jiaotong University, Xi’an, Shaanxi 710049, China Received May 29, 2010

Downloaded via IOWA STATE UNIV on January 11, 2019 at 01:54:33 (UTC). See https://pubs.acs.org/sharingguidelines for options on how to legitimately share published articles.

Contents 1. Introduction 2. Basic Principles of Photocatalytic Hydrogen Generation 2.1. Fundamental Mechanism of Photocatalytic Hydrogen Generation 2.2. Main Processes of Photocatalytic Hydrogen Generation 2.3. Evaluation of Photocatalytic Water Splitting 2.3.1. Photocatalytic Activity 2.3.2. Photocatalytic Stability 3. UV-Active Photocatalysts for Water Splitting 3.1. d0 Metal Oxide Photocatalyts 3.1.1. Ti-, Zr-Based Oxides 3.1.2. Nb-, Ta-Based Oxides 3.1.3. W-, Mo-Based Oxides 3.1.4. Other d0 Metal Oxides 3.2. d10 Metal Oxide Photocatalyts 3.3. f0 Metal Oxide Photocatalysts 3.4. Nonoxide Photocatalysts 4. Approaches to Modifying the Electronic Band Structure for Visible-Light Harvesting 4.1. Metal and Nonmetal Doping 4.1.1. Metal Ion Doping 4.1.2. Nonmetal-Ion Doping 4.1.3. Metal/Nonmetal-Ion Codoping 4.2. Controlling Band Structure through Solid Solutions 4.2.1. (Oxy)sulfide Solid Solutions 4.2.2. Oxide Solid Solutions 4.2.3. Oxynitride Solid Solutions 4.3. Dye Sensitization to Harvest Visible Light 4.3.1. Sensitization Using Ruthenium Complex Dyes 4.3.2. Sensitization Using Other Transition-Metal Complex Dyes 4.3.3. Sensitization Using Metal-Free Dyes 4.4. Developing Novel Single-Phase Visible-Light-Responsive Photocatalysts 4.4.1. d-block Metal Oxides 4.4.2. p-block Metal Oxides 4.4.3. f-block Metal Oxides 4.4.4. Miscellaneous Photocatalysts

6503 6505 6505 6505 6507 6507 6507 6507 6507 6507 6514 6517 6518 6518 6518 6518 6519 6519 6519 6529 6531 6532 6532 6533 6534 6535 6535 6536 6536 6537 6538 6539 6540 6541

* Corresponding author: Xiaobo Chen. E-mail: [email protected] (Xiaobo Chen); [email protected] (Shaohua Shen); lj-guo@ mail.xjtu.edu.cn (Liejin Guo); [email protected] (Samuel S. Mao). † Lawrence Berkeley National Laboratory. ‡ Xi’an Jiaotong University.

5. Approaches for Efficient Photogenerated Charge Separation 5.1. Cocatalyst Loading 5.1.1. Noble Metal Cocatalysts 5.1.2. Transition-Metal Oxide Cocatalysts 5.1.3. Nonmetal-Oxide Cocatalysts 5.2. Semiconductor Combinations 5.3. Modification of Crystal Structure and Morphology 5.3.1. Modification of Crystal Structure 5.3.2. Modification of Size and Morphology 6. Photocatalytic Hydrogen Generation Systems 6.1. Hydrogen Generation Systems Containing Sacrificial Reagents 6.1.1. Inorganic Sacrificial Reagent Systems 6.1.2. Organic Sacrificial Reagent System 6.2. Overall Water-Splitting Systems 6.2.1. Pure Water-Splitting System 6.2.2. Biomimetic Z-Scheme Water-Splitting System 7. Summary and Prospects 8. Acknowledgments 9. References

6541 6541 6542 6542 6543 6544 6547 6547 6548 6552 6552 6552 6555 6556 6556 6556 6557 6558 6558

1. Introduction Because of its high energy capacity and environmental friendliness, hydrogen has been identified as a potential energy carrier in many low greenhouse gas (GHG) energy scenarios.1,2 In a proposed hydrogen energy system,3 hydrogencontaining compounds such as fossil fuels, biomass, or even water are potential sources of hydrogen.4-11 When hydrogen is derived from hydrocarbons such as fossil fuels or biomass, CO2 capture and sequestration are requirements in a low GHG scenario.12-14 On the other hand, hydrogen produced from water does not present the challenge of unwanted emissions at the point of conversion, but it does require that energy be supplied from an external resource.15 If this energy can be obtained from a renewable energy source such as solar energy, hydrogen can then be considered a green energy alternative capable of powering everything from laptops to submarines. Figure 1 shows a diagram of photocatalytic hydrogen generation in the hydrogen energy system. Such an approach to energy production is one that exhibits due concern for environmental issues and that is becoming increasingly relevant in our world.16,17 However, the technology to produce hydrogen in a cost-effective, low-GHG manner has not yet been developed. Since the discovery of hydrogen evolution through the photoelectrochemical splitting of water on n-type TiO2

10.1021/cr1001645  2010 American Chemical Society Published on Web 11/10/2010

6504 Chemical Reviews, 2010, Vol. 110, No. 11

Dr. Xiaobo Chen is at Lawrence Berkeley National Laboratory. He obtained his Ph.D. Degree in Chemistry from Case Western Reserve University. His research interests include materials and devices development, renewable energy science and technology, environmental pollution, and health.

Dr. Shaohua Shen is an assistant professor at Xi’an Jiaotong University, China. He obtained his Ph.D. Degree in Thermal Engineering from Xi’an Jiaotong University in 2010. During 2008-2009, he worked as a guest researcher at Lawrence Berkeley National Laboratory, U.S.A. His research interests include photocatalysis, photoelectrochemistry, and the related materials and devices development.

Chen et al.

Dr. Samuel S. Mao is a career staff scientist at Lawrence Berkeley National Laboratory and an adjunct faculty at The University of California at Berkeley. He obtained his Ph.D. degree in Engineering from The University of California at Berkeley in 2000. He is leading a multidisciplinary research team developing solar-active materials and devices and investigating fundamental energy conversion processes.

development of the necessary semiconductor photocatalysts has undergone considerable research. Over the past 40 years, many photocatalysts reportedly exhibited high photocatalytic activities for splitting water into a stoichiometric mixture of H2 and O2 (2:1 by molar ratio) in the ultraviolet (UV) light region. These include La doped NaTaO3,20 Sr2M2O7 (M ) Nb, Ta),21 La2Ti2O7,22 K2La2Ti3O10,23 and β-Ge3N4,24 among others. Of particular note is the NiO/NaTaO3:La photocatalyst, which shows the highest activity with a quantum yield amounting to 56% at 270 nm.20 However, these oxide photocatalysts are only active under UV irradiation. With respect to the solar spectrum, only a small fraction (ca. 4%) of the incoming solar energy lies in the ultraviolet region, whereas the visible light in the solar spectrum is far more abundant (ca. 46%). It is essential, therefore, as an alternative to UV-active photocatalysts to develop visible-light-driven photocatalysts that are stable and highly efficient for the practical, large-scale production of hydrogen using solar energy. Over the recent years, continuing breakthroughs have been made in the development of novel visible-light-driven photocatalysts, leading to the enhancement of photocatalytic activity for water splitting and inspiring great enthusiasm. A large number of semiconductor materials have been developed as photocatalysts for water splitting to hydrogen under visible-light irradiation. A significant process has been achieved on semiconductorbased photocatalytic hydrogen generation through water

Dr. Liejin Guo is a professor and the director of the State Key Laboratory of Multiphase Flow in Power Engineering in Xi’an Jiaotong University, China. He obtained his Ph.D. Degree in Engineering Thermophysics from Xi’an Jiaotong University in 1989. His research interest includes multiphase flow, heat transfer, and renewable energy technologies.

electrodes,18 the technology of semiconductor-based photocatalytic water splitting to produce hydrogen using solar energy has been considered as one of the most important approaches to solving the world energy crisis.19 Hence, the

Figure 1. Schematic diagram of photocatalytic hydrogen generation in the hydrogen energy system.

Photocatalytic Hydrogen Generation

splitting over the past several decades,25-31 and many excellent reviews have been published.32-62 In this review, we aim to put together the research effort having been made so far, with a view of providing a good reference and inspiring new ideas for tackling this important challenge. Starting with a brief introduction to semiconductor-based photocatalysts for hydrogen generation from water splitting, we overview the development of high-efficiency, visiblelight-driven photocatalysts. A number of synthetic and modification techniques for adjusting the band structure to harvest visible light and improve the charge separation in photocatalysis are discussed. Photocatalytic systems for water splitting are also reviewed and classified into two main kinds: sacrificial reagent-containing water-splitting systems and overall water-splitting systems.

2. Basic Principles of Photocatalytic Hydrogen Generation 2.1. Fundamental Mechanism of Photocatalytic Hydrogen Generation In Fujishima and Honda’s pioneering work, the electrochemical cell they constructed for the decomposition of water into hydrogen and oxygen is shown in Figure 2.18 When the surface of the TiO2 electrode was irradiated by UV light, as a result of a water oxidation reaction, oxygen evolution occurred at the TiO2 electrode. Concomitant reduction led to hydrogen evolution at the platinum black electrode. This concept, which emerged from the use of photoelectrochemical cells with semiconductor electrodes, was later applied by Bard to the design of a photocatalytic system using semiconductor particles or powders as photocatalysts.63-65 A photocatalyst absorbs UV and/or visible (Vis) light irradiation from sunlight or an illuminated light source. The electrons in the valence band of the photocatalyst are excited to the conduction band, while the holes are left in the valence band. This, therefore, creates the negative-electron (e-) and positive-hole (h+) pairs. This stage is referred to the semiconductor’s “photo-excited” state, and the energy difference between the valence band and the conduction band is known as the “band gap”. This must correspond to the wavelength of the light for it to be effectively absorbed by the photocatalyst. After photoexcitation, the excited electrons and holes separate and migrate to the surface of photocatalyst. Here, in the photocatalytic water-splitting reaction, they act

Chemical Reviews, 2010, Vol. 110, No. 11 6505

Figure 3. Fundamental principle of semiconductor-based photocatalytic water splitting for hydrogen generation.

as reducing agent and oxidizing agent to produce H2 and O2, respectively. A schematic representation of the principle of the photocatalytic system for water is depicted in Figure 3. Water splitting into H2 and O2 is an uphill reaction. It needs the standard Gibbs free energy change ∆G0 of 237 kJ/mol or 1.23 eV, as shown in eq 1.

1 H2O f O2 + H2 ; 2

∆G ) +237 kJ/mol

(1)

Therefore, the band gap energy (Eg) of the photocatalyst should be >1.23 eV (290 nm 330 nm quartz filter

incident light pure water pure water pure water pure water pure water pure water pure water NaOH NaOH pure water NaOH pure water pure water pure water pure water pure water NaOH pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water RbOH CsOH pure water pure water CH3OH CH3OH CH3OH CH3OH CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 pure water CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 Ce4+ pure water

aqueous reaction solution

RuO2/∼100

NiOx/985 NiO/19 800 NiO/19 000 NiO/18 600 NiOx/5290 NiOx/5190 NiOx/5290 NiO/782 NiO/974 4 NiO/72 NiO/960 NiO/629 NiO/15 11 NiOx/92 NiO/340 NiO/5024 748 770 176 NiOx/235 NiOx/6 NiOx/53 NiO/1880 NiO/292 RuOx/200 NiOx/3540 NiOx/1465 NiOx/885 NiOx/900 NiOx/445 NiOx/150 NiO/2388 NiO/64 NiO/7110 2460 NiOx/340 NiOx/578 NiOx/23.5 NiOx/328 NiO/70 NiOx/232.3 NiOx/65.7 41.8 33.6 NiO/1089 Pt/7 Pt/84.4 Pt/389.6 1500 11 300 550 RuO2/96 Pt/9 Pt/18 Pt/98.3 Pt/2 Pt/0 Pt/23.3 Pt/3.3 Pt/0.01

co-catal./H2

300 600 250 RuO2/48 8 218 161.7 193.3 35.7 4.3 19.3 2.1 15.9 RuO2/∼50

NiO/1444 NiO/4 NiO/3621 1110 NiOx/170 NiOx/257.5 NiOx/3.5 NiOx/160 NiO/15.8 NiOx/115 NiOx/29.3 20.5 16

NiO/32 NiO/490 NiO/303 NiO/6 4 NiOx/46 NiO/166 NiO/2476 384 358 22.8 NiOx/126.5 NiOx/3 NiOx/28.5 NiO/918 NiO/132 RuOx/78.8 NiOx/1665 NiOx/810 NiOx/405 NiOx/455 NiOx/265

NiOx/398 NiO/9660 NiO/9400 NiO/9380 NiOx/2580 NiOx/2510 NiOx/2630 NiO/390 NiO/452

co-catal./O2

activity (µmol · h-1 · g-1)

8 (300 nm >300 nm quartz filter quartz filter quartz filter quartz filter quartz filter quartz filter quartz filter quartz filter quartz filter quartz filter >200 nm >300 nm Pyrex filter Pyrex filter Pyrex filter quartz filter quartz filter quartz filter quartz filter

quartz filter

incident light

b

pure water pure water ethanol pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water pure water CH3OH/AgNO3 pure water pure water pure water CH3OH/AgNO3 CH3OH/AgNO3 CH3OH/AgNO3 pure water pure water pure water pure water pure water pure water pure water pure water pure water H2SO4 H2SO4 pure water pure water pure water Na2SO3 Na2S methanol pure water


c

70 800 RuO2/295 20a RuO2/∼3.6 RuO2/∼84 RuO2/∼28 RuO2/∼28 RuO2/∼4.8 RuO2/∼32 RuO2/∼26 RuO2/∼5.6 RuO2/∼12 RuO2/∼30.4 RuO2/∼16 Pt/8200 RuO2/∼48 RuO2/∼84 RuO2/∼104 Pt/∼30a Pt/0a Pt/∼50a Ni/338 Ni/4100 Ni/950 Ni/640 Ni/765 Ni/534 46.8 40.7 NiOx/100.4 RuO2/∼3600 Rh2-xCrxO3/63.3 RuO2/∼750 RuO2/∼250 RuO2/∼587.5 Pt/34 037.5 Pt/100 650 32.8

co-catal./H2

16.4

RuO2/∼1.2 RuO2/∼40 RuO2/∼12 RuO2/∼12 RuO2/∼2 RuO2/∼14 RuO2/∼8 RuO2/∼0.8 RuO2/∼4 RuO2/∼12 RuO2/∼6.8 2500 RuO2/∼16 RuO2/∼40 RuO2/∼52 ∼25a ∼60a ∼7a Ni/171 Ni/2200 Ni/550 Ni/282 Ni/348 Ni/256 22.9 20.7 NiOx/53.4 RuO2/∼1600 Rh2-xCrxO3/31.7 RuO2/∼362.5 RuO2/∼125 RuO2/∼287.5

15 250 RuO2/130

co-catal./O2


90 (313 nm)

0.628 (>390 nm) 6.81 (320 nm) 9 (300 nm) 0.7 (300-340 nm)

∼20

38.7

QY (%)

The unit of H2/O2 evolution rate is µmol · h , as the weight of photocatalyst has not been given in the reference. Mercury lamp. Xenon lamp. d Fluorescent lamp. e Metal halide lamp.

-1

impregnation method polymerized complex method electrodeposition mehtod solid-state reaction precipitation, calcination precipitation, calcination precipitation, calcination solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction hydrothermal, calcination solid-state reaction solid-state reaction solid-state reaction solid-state reaction Kanto Chemicals rare metallic high-purity chemical impregnation, calcination impregnation, calcination impregnation, calcination impregnation, calcination impregnation, calcination solid-state reaction solid-state reaction solid-state reaction NH3 nitridation NH3 nitridation NH3 nitridation NH3 nitridation NH3 nitridation precipitation Kojundo Chemical Laboratory Schumann emulsion impregnation method

Ce-MCM-41 BaCeO3 VO2 NaInO2 CaIn2O4 SrIn2O4 Sr0.93Ba0.07InO4 LaInO3 YxIn2-xO3 NaSbO3 CaSb2O6 Ca2Sb2O7 Sr2Sb2O7 Sr2SnO4 SrSnO3 ZnGa2O4 Zn2GeO4 LiInGeO4 Ga1.14In0.86O3 In2O3 β-Ga2O3 Ga2O3 Ga2O3:Zn Ga2O3:Ca Ga2O3:Sr Ga2O3:Ba Ga2O3:Ta Bi2GaVO7 Bi2YVO8 Zn-Lu2O3/Ga2O3 Ge3N4 GaN GaN:Mg GaN:Zn GaN:Be ZnS InP AgBr/SiO2 H4SiW12O40/SiO2

a

synthetic method

photocatalyst

Table 1. Continued

reference 271 272 250 258, 260 259-262 259-262 260 259 257 261, 263 263 263 263 261 268 264 265 266 256 256 256 253, 254 254 254 254 254 254 251 252 255 24, 277-279 275 276, 759 276, 759 759 273, 364 274 280 249

6512 Chemical Reviews, 2010, Vol. 110, No. 11 Chen et al.


with HCl.70 The addition of either NaOH or Na2CO3 was found to be effective for water splitting using the Pt/TiO2 photocatalyst.71,75,78 When TiO2 was doped with metal ions, the photocatalytic activity for water splitting was effectively enhanced. Chae et al. reported that, whereas Ga doped TiO2 powder could split pure water stoichiometrically under UV irradiation, pure TiO2 did not show any activity.79 The Ni2+ doping enhanced the photoactivity of the TiO2 for hydrogen production from an aqueous methanol solution.80 Sn/Eu codoped TiO2 exhibited a high activity for hydrogen generation with a quantum efficiency of ∼40% with Pd as the cocatalyst under the irradiation from a fluorescent lamp.81 Zalas and La studied the effect of lanthanide doping on the photocatalytic activity of TiO2.82 The best performance for hydrogen production from an aqueous methanol solution was obtained for the TiO2 containing 0.5 mol % of Gd oxide as the dopant. The UV-driven photocatalytic activity of TiO2 was also improved by combining it with a second oxide semiconductor. All of the mixed oxides with heterophasestructures, SnO2/TiO2,83 ZrO2/TiO2,84 CuxO/TiO2,85-87 AgxO/ TiO2,88-90 and MTiO3/TiO2 (M ) Ca, Sr, Ba),91 displayed higher rates of photocatalytic hydrogen evolution from aqueous solutions containing electron donors other than TiO2 alone. With Pt as a cocatalyst, the Ti/B binary oxide stoichiometrically decomposes pure water under UV irradiation.92,93 When TiO2 nanoclusters were dispersed in the mesoporous structures of MCM-41 and MCM-48, the formed Ti-MCM-4194 and Ti-MCM-4895 showed much higher photocatalytic activity for hydrogen evolution under UV irradiation than bulk TiO2. Many white titanates are known to work as efficient photocatalysts for water splitting under UV irradiation. Shibata et al. reported that the layered titanates, Na2Ti3O7, K2Ti2O5, and K2Ti4O9, were active in photocatalytic H2 evolution from aqueous methanol solutions even without the presence of Pt cocatalyst.96 These layered titanates, consisting of titanium oxide layers and interlayers, can be modified using ion-exchange reactions.96,97 Of the materials studied, the H+-exchanged K2Ti2O5 exhibited a high activity with a quantum yield of up to ca. 10%. After being pillared with SiO2 in the interlayers, K2Ti4O9 showed an enhanced photocatalytic acitivity for H2 evolution from CH3OH/H2O mixtures. This is in agreement with an increase in the surface area.98 The Na2Ti2O5 titanate nanotube material with a nickel complex intercalated into the interlayers also showed a high photocatalytic activity for H2 evolution from water/methanol solutions under UV irradiation.99 Kudo and Kondo found that a range of Cesium compounds, Cs2TinO2n+1 (n ) 2, 5, 6), with layered structures showed photocatalytic activities for H2 and O2 evolution from aqueous solutions.100 The Cs2Ti2O5 with a five-coordinate structure consisting of TiO5 units was more active than Cs2Ti5O11 and Cs2Ti6O13 with six-coordinate structures consisting of TiO6 units. The unsaturated coordination state of the five-coordinate structure worked as the active sites of catalytic reactions and contributed to the photoactivity. The photoactivity of Cs2Ti2O5 was also greatly enhanced by the H+-exchange reaction. Inoue and co-workers investigated a series of alkali-metal titanates with a chemical formula of M2TinO2n+1 (M ) Na, K, Rb and n ) 2, 3, 4, 6) as photochemical water-splitting catalysts.101-104 The alkaline metal atoms, M, in M2Ti6O13 showed a great effect on the photocatalytic activity for water splitting. Interestingly, RuO2/M2Ti6O13 (M ) Na, K, and Rb) with rectangular tunnel structures showed higher photocata-


lytic activity than RuO2/Cs2Ti6O13 with a layered structure. The activity increased in the order of Na > K > Rb > Cs. Kohno et al. reported that, in a photocatalytic system of ruthenium oxide-deposited barium titanates (BaTi4O9, Ba2Ti9O20, Ba4Ti13O30, and Ba6Ti17O40), only RuO2/BaTi4O9 was active in water decomposition.105 The pentagonal prism tunnel structure of RuO2/BaTi4O9 gave rise to a higher photocatalytic activity than RuO2/K2Ti4O9 with a zigzag layer structure. It is believed that the tunnel structure was responsible for the high dispersion of the RuO2 particles.104,106,107 The method of catalyst preparation also appears to play a role in the final activity. For example, BaTiO3 synthesized with a polymerized complex method exhibited enhanced photocatalytic activity when compared to the materials prepared by traditional solid-state reaction method.108 This was due to the larger surface area. Domen and co-workers reported that a NiO-loaded SrTiO3 powder was capable of decomposing pure water as well as water vapor into H2 and O2 under UV irradiation.109-114 The activity of the photocatalyst was increased considerably by a pretreatment in H2 and using a concentrated NaOH solution for the photocatalytic reaction.111 The photocatalytic activity of SrTiO3 was also greatly improved by using a modified preparation method115 or a suitable concentration of metal cations doping (such as La3+,116 Ga3+,117 and Na+ 117). Some derivatives, such as Sr3Ti2O7 and Sr4Ti3O10, were also found to be active in water decomposition when loaded with NiO as the cocatalysts.118,119 Mizoguchi et al. reported that platinized CaTiO3 powder, with band gap of 3.5 eV estimated from optical absorption edge, exhibited a high photocatalytic activity under UV irradiation.120 By doping with Zr4+ to form a CaTi1-xZrxO3 solid solution, the activity was further increased. Quantum yields of up to 1.91% and 13.3% for H2 evolution from pure water and aqueous ethanol solution, respectively, were reported.121 Lee and co-workers investigated a series of perovskites whose layers were integrated of the intergrowth with the same elements (La and Ti) but had different layer thicknesses.122-124 La2TiO5, La2Ti3O9, and La2Ti2O7, which had layered structures made up of slabs of 1, 3, and 4 units, respectively, showed much higher photocatalytic activities under UV irradiation than bulk LaTiO3. Alkaline earth component-doping (Ba, Sr, and Ca) was shown to improve the photoactivities of La2Ti2O7. In particular, the NiOmodified Ba-doped La2Ti2O7 proved extremely active for overall water splitting with a quantum yield close to 50% on condition that alkaline hydroxide was introduced into the reaction system as an external additive.125 The activity of La2Ti2O7 was highly enhanced by synthesizing the catalyst using the polymerized approach instead of the solid-state reaction method.22,126 In contrast, La2Ti2O7, Ln2Ti2O7 (Ln ) Pr, Nd) with a layered structure was also active for water splitting but exhibited lower activities, with the activity decreasing in the order La2Ti2O7 . PrLaTi2O7 > Pr2Ti2O7 > NdLaTi2O7 > Nd2Ti2O7.127 The use of titanate R2Ti2O7 (R ) Y, Eu-Lu) with pure cubic-pyrochlore structure as water-splitting photocatalysts was first reported in 2004 by Abe’s group.128 Among them, NiOx-loaded Y2Ti2O7 demonstrated the most efficient evolution of H2 and O2 in a stoichiometric ratio from pure water under UV irradiation. Y2Ti2O7 photocatalysts, with better crystallinity and higher activity, were obtained by the addition of excess Y in the polymerized complex synthetic procedure.129,130 They also found that the high photocatalytic activ-


ity observed for overall water splitting over R2Ti2O7 (R ) Y, Gd) was related to the increased mobility of the electrons and holes caused by the corner-shared octahedral TiO6 network in these materials.131 Uno et al. also studied the photocatalytic activities for hydrogen evolution using Ln2Ti2O7 (Ln ) La, Pr, Nd, Sm, Gd, Dy, Ho, Er, and Yb).132 However, only La2Ti2O7 and Sm2Ti2O7 showed detectable photocatalytic hydrogen evolution, and even that was a small rate. Miseki et al. studied the photocatalytic properties of ALa4Ti4O15 (A ) Ca, Sr, and Ba) with a (111) plane-type layered perovskite structure.133 Of these, NiOx-modifed BaLa4Ti4O15 showed the highest activity for water splitting, with a quantum yield of 15% at 270 nm. The highly donordoped (110) layered perovskite La4CaTi5O17 was found to be an efficient photocatalyst for overall water splitting with quantum yield as high as 20% under UV irradiation.134 The spontaneously hydrated layered perovskites with a general formula of A2-xLa2Ti3-xNbxO10 (A ) interlayer cations such as K, Rb, Cs; x ) 0-1) were found to be efficient photocatalysts for water decomposition under UV irradiation.135-137 NiO/Rb2La2Ti3O10 produced H2 and O2 from a RbOH aqueous solution with quantum yield up to 5%. Suitable modification techniques such as cocatalyst loading, using Ni or Au,138,139 metal-ion doping (Zn2+ doping),140 and alternative synthetic methods23,141 all led to the enhanced activity of K2La2Ti3O10. The polymerized complex synthesis method was also utilized to prepare the high-purity stoichiometric KTiNbO5 photocatalyst, which was demonstrated with increased activity after NiO loading.142 For KLaTiO4, Zr4+ doping had a positive effect on the photocatalytic activity in a water-splitting reaction, giving rise to a quantum yield as high as 12.5%.143 Sekine et al. were the first to examine the photocatalytic reactions on the ion-exchangable layered titanoniobate compounds, CsNbTi2O7 and CsNbTiO5.144 They found that the H+-exchanged forms of those compunds work as efficient photocatalysts for H2 or O2 evolution from an aqueous solution containing methanol or silver nitrate under UV irradiation. Members of the aurivillius-type layered perovskites (Bi2O2)2+(An-1BnO3n+1)2- (A ) Ba, Bi, etc.; B ) Ti, Nb, etc.), Bi4Ti3O12, BaBi4Ti4O15, and Bi3TiNbO9 evolved H2 and O2 from aqueous methanol and AgNO3 solutions, respectively.145 He and Yang investigated the photocatalytic activity for hydrogen production over another layered perovskite KBi3PbTi5O16 under UV irradiation.146 It was found that the photocatalyst prepared by the polymerized complex method showed much higher activity than that prepared by the solid-state reaction method. In addition, the rate of hydrogen evolution was greatly improved and affected by the addition of Ce(SO4)2 in an aqueous suspension. Sayama and Arakawa were the first to find that the photocatalytic decomposition of pure water proceeded over ZrO2 powder without any loaded metals as cocatalysts under UV irradiation.78,147,148 The activity was affected significantly by the pressure of the reaction system, the nature of the additive, and the pH of the solution. Specifically, the addition of Na2CO3 or NaHCO3 led to a remarkable increase in the activity and stability of the gas-evolution rate. However, the activity decreased when metals such as Pt, Au, Cu, and RuO2 were loaded onto the surface of the ZrO2. It was presumed that the large electronic barrier height of the semiconductormetal junction prevented the migration of electrons from ZrO2 to the metal. This would lead to the loaded metals,

Chen et al.

possibly blocking the reaction sites on the ZrO2. Reddy et al. revealed that the photocatalytic activity of ZrO2 prepared by the precipitation method was highly dependent on the hydrolyzing agent used.149 The highest photocatalytic activity was obtained for the ZrO2 with the highest surface area when KOH was used as the hydrolyzing agent. Zou et al. reported that a clean and direct metal-support interface of a NiOloaded ZrO2 photocatalyst could be obtained using a plasma method.150 In photocatalytic reactions, this interface proved more efficient for the charge separation and transfer, which in turn led to the higher photocatalytic activity for water splitting using NiO/ZrO2 by the plasma treatment than that prepared with the traditional thermal treatment. Compared to the conventional bulk ZrO2, the photocatalytic watersplitting activity was greatly enhanced by the high dispersion of ZrO2 into the amorphous wall of MCM-41.151 BaZrO3 with a cubic perovskite structure produced hydrogen efficiently with a quantum yield up to 3.7% from pure water without the assistance of any cocatalysts under UV irradiation.152 The high photoactivity of BaZrO3 was attributed to the highly negative potential of the photoinduced electrons, the 180° Zr-O-Zr bond angle, and the large dispersion of the conduction band edge composed of Zr 4d orbitals. When the Zr element was partially substituted by Sn, the photocatalytic activity for water splitting was obviously improved.153 Uno et al. investigated the photocatalytic activities for hydrogen evolution of a series of lanthanide zirconium oxides, Ln2Zr2O7 (Ln ) La, Ce, Nd and Sm).154 Under the illumination of a 500-W Xenon lamp, hydrogen gas was clearly evolved in a distilled water suspension of La2Zr2O7, Sm2Zr2O7, and Nd2Zr2O7. On the other hand, Ce2Zr2O7 showed no photocatalytic activity because of its lower conduction band level. After modification with Pt as a cocatalyst, mesoporous zirconium-titanium phosphates demonstrated considerable activity in photocatalytic water decomposition.155 The H2 production rate was gradually increased on the addition of Zr, and the maximum H2 evolution was observed for the Zr0.5Ti0.5PO4 material. Furthermore, the use of sodium carbonate as a pH adjuster was essential and significant for hydrogen generation and also provided stability for the photocatalytic reaction system. A zirconium phosphate/ phosphonate compound with quantum yield of 4% was developed to produce hydrogen photochemically from water. It was based only on the ultraviolet portion of the spectrum in the presence of a sacrificial reductant (EDTA).156

3.1.2. Nb-, Ta-Based Oxides Pure Nb2O5, with a band gap of ca. 3.4 eV determined from the threshold of UV-vis absorption, is not active for pure water splitting under UV irradiation.157 After modification with Pt as a cocatalyst, however, it can efficiently produce H2 from aqueous solutions containing methanol as an electron donor.158 Mesoporous Nb2O5, synthesized via an evaporation-induced self-assembly method, demonstrated a photocatalytic activity 20 times higher for hydrogen evolution than a bulk Nb2O5 without any porosity.158 Intercalation of In2O3 into the mesoporous structure further increased the photoactivity of mesoporous Nb2O5 by 2.7 times.159 Besides Nb2O5, a large number of niobates can produce H2 and O2 via water splitting upon UV irradiation. In 1986, Domen and co-workers developed K4Nb6O17 as the first example of a niobate photocatalyst that showed high and stable activity for H2 evolution from aqueous methanol


solution without any assistance from other materials such as the noble metals.160,161 This niobate is composed of layers of niobium oxide sheets, in which potassium ions are located in two different kinds of interlayers. One type of interlayer contains water molecules and potassium ions, and the other contains only potassium ions. The potassium ions between the niobium oxide layers can be exchanged with many other cations including transition metal ions. The activities of catalysts exchanged with H+, Cr3+, and Fe3+ ions were higher than the original K4Nb6O17. Of particular note is the H+exchanged K4Nb6O17, which showed the highest activity for H2 evolution from an aqueous methanol solution. Its quantum yield was up to ca. 50% at 330 nm.160,162 After modification with NiO,163-166 Au,167 Pt,168,169 and Cs170 as cocatalysts, K4Nb6O17 was quite efficient for simultaneous hydrogen and oxygen evolution from pure water. Upon the addition of alkaline hydroxide (KOH, NaOH) into the aqueous impregnation solution, the activity of the NiO/K4Nb6O17 photocatalyst for overall water splitting was enhanced, with a quantum efficiency of 5.3% (330 nm) under optimum conditions.166 Rb4Nb6O17, which has the same layered structure, exhibited a high activity for photocatalytic water splitting to form H2 and O2 under band gap irradiation. The quantum efficiency at 330 nm was ca. 10% in the initial stage of the reaction over the NiO(0.1 wt %)-Rb4Nb6O17 photocatalyst.171 When doped with Ta2O5, layered compounds of the type A4TaxNb6-xO17 (A ) K or Rb, x ) 2, 3, and 4) were able to decompose water stoichiometrically after the pretreatment of H2 reduction and O2 reoxidation at high temperatures. This was possible even in the absence of any loaded metals as cocatalysts.157 Some other alkaline-metal niobates such as ANbO3 (A ) Li, Na, K)172-174 and Cs2Nb4O11175 also catalyzed H2 and/or O2 evolution from water under UV irradiation, but only after modification with Pt, RuO2, or NiO. Ikeda et al. found that tungsten-containing alkaline niobates with a defect pyrochlore structure, ANbWO6 (A ) Rb, Cs), and loaded with nickel oxide, showed photocatalytic activity for overall water splitting under UV irradiation.176 The conduction bands of the materials were thought to be composed of the W5d orbital hybridized with the Nb5d orbital. Photocatalytic water splitting over the alkaline-earth niobates have been studied by various researchers. The related strontium niobates SrNb2O6,177 Sr2Nb2O7,21,134,177 and Sr5Nb4O15133 exhibited efficient photocatalytic activities for hydrogen and oxygen production from pure water under UV irradiation. In particular, Sr2Nb2O7 with a highly donor-doped (110) layered perovskite structure gave quantum yields as high as 23%.134 The activity of Sr2Nb2O7 was further enhanced to give a quantum yield of 32%, by using a hydrothermal synthetic process that produced a 1D nanostructure with larger Brunauer-Emmett-Teller (BET) surface areas.177 In comparison, the quantum yield of Ca2Nb2O7 was 7%.134 Ba5Nb4O15 with a layered perovskite structure was studied by Kudo and co-workers.133,134 It gave a 17% quantum yield at 270 nm for water splitting when loaded with NiO cocatalysts. Partial substitution of Nb5+ with Zn2+ gave the resulting BaZn1/3Nb2/3O3 with a distorted perovskite structure, which showed favorable photocatalytic activity under UV irradiation.178,179 Domen and co-workers first reported a novel DionJacobsen series of ion-exchangeable niobates, A(Mn-1NbnO3n+1) (A ) Na, K, Rb, Cs; M ) La, Ca, Sr, etc.), with layered perovskite structures that showed unique photocata-


lytic activities. This was especially true for the H+-exchanged forms, for H2 evolution from aqueous alcohol solutions as well as O2 evolution from an aqueous silver nitrate solution.38,180 For example, KSr2Nb3O10 produced hydrogen at a rate of 0.11 mmol/h/g. After cation exchange with protons, the rate of HSr2Nb3O10 increased to 43 mmol/h/g.38 The related layered niobate K2.33Sr0.67Nb5O14.335 was also reported by Wu and co-workers to show much higher photoactivity for hydrogen evolution after a proton-exchange reaction.181 They further reported that other modifications for proton-exchanged H(Mn-1NbnO3n+1) (M ) La, Ca, Sr, etc.), such as metal-ion doping (La3+,182 In3+183, and Mo6+184 doped into HCa2Nb3O10 and H2LaNb2O7, respectively), efficiently improved the photocatalytic hydrogen evolution from aqueous methanol solutions. When H2LaNb2O7 was synthesized using a polymerized complex method, it showed higher activity for water splitting than the same material prepared by a solid-state reaction.185 Ebina and co-workers synthesized a restacked aggregate of exfoliated nanosheets of [Ca2Nb3O10]- by flocculation with NaOH and KOH aqueous solutions. Under UV irradiation, the restacked aggregates, with a 10-fold enhancement of the surface area, showed higher activities for photocatalytic hydrogen evolution than the KCa2Nb3O10 starting compound;186 overall photocatalytic splitting of water was achieved when RuOx was intercalated between the layers during the exfoliation-restacking route.187 After exfoliation using tetrabutylammonium hydroxide, the restacked TBAx[H1-xCa2Nb3O10] sheets loaded with Pt cocatalysts produced hydrogen from pure water with a quantum efficiency of 7.5%. However, no oxygen was observed. Transient absorption measurements of the nanosheets revealed charge separation on a nanosecond time scale.188 SiO2pillared HCa2Nb3O10, prepared from the layered perovskite KCa2Nb3O10 via alkylammonium ion-intercalated HCa2Nb3O10, showed much higher photocatalytic activity of H2 evolution from aqueous solutions of long-chain alcohols.189,190 This effect was attributed to the expanded interlayer space facilitating the intercalation of such alcohols that could then serve as efficient electron donors. In 2008 a new member of the Dion-Jacobsen perovskites, H2Ca4Nb6O20, was reported to be active for H2 evolution in the presence of methanol as a sacrificial agent under UV irradiation.191 When Nb was partially substituted by Ta, the resulting H2Ca4Ta2Nb4O20 showed the best photocatalytic activity. The photocatalytic H2 evolution rate was 8.5 mmol/h/g. Abe and co-workers investigated the effect of crystal structure on water splitting using R3NbO7 (R ) Y, Yb, Gd, La).131,192 Only La3NbO7, which has an orthorhombic weberite structure and which formed a NbO6 octahedral network that increased the mobility of both electrons and holes, was active for the photocatalytic water-splitting reaction. On the other hand, La1/3NbO3, crystallizing in an A-site deficient perovskitetype structure instead, catalyzed H2 evolution with a Pt cocatalyst from CH3OH/H2O solution. In addition, O2 evolution from AgNO3 aqueous solution under UV irradiation was observed.193 Kudo et al. reported a new ZnNb2O6 photocatalyst consisting of d10 and d0 metal ions.194 Under UV irradiation, the activity of the native ZnNb2O6 was negligible, whereas NiO-loaded ZnNb2O6 showed the high activity after a H2reduction and O2-oxidation pretreatment. Chen and coworkers prepared a new series of layered perovskite photocatalysts, ABi2Nb2O9 (A ) Ca, Sr, Ba), by the conventional


solid-state reaction method.195 Under UV irradiation, these photocatalysts showed photocatalytic activity for both H2 and O2 evolution from aqueous solutions containing sacrificial reagents (methanol and Ag+). The activities decreased in the order of SrBi2Nb2O9 > BaBi2Nb2O9 > CaBi2Nb2O9. Zou and co-workers found that the compounds M2BiNbO7 (M ) In3+, Ga3+) with pyrochlore structures were sensitive to UV irradiation and had the ability to split water stoichiometrically to produce H2 and O2.196 On the other hand, Bi2MNbO7 (M ) Al3+, Ga3+, In3+) with the same pyrochlore structure only evolved H2 or O2 in the presence of CH3OH or Ce(SO4)2 as sacrificial agents.197 The photocatalytic hydrogen production over NiO/Bi2AlNbO7 was efficiently improved with La3+ doping.198 In comparison, Bi2MNbO7 (M ) Y3+, Ce3+, Gd3+, Sm3+, Nd3+, Pr3+, and La3+) evolved H2 at only a small rate from pure water under UV irradiation.199 The increase of ion radius of M3+ in Bi2MNbO7 led to the decrease in the photocatalytic activity. The narrower band gap formed by the smaller ion radius of M3+ suggested easier excitation for an electron from the valence band to the conduction band in the oxide semiconductor. BiNbO4 with a triclinic structure produced only a small amount of hydrogen from pure water under UV irradiation. When doped with Ta, the resulting BiTa0.8Nb0.2O4 had an orthorhombic structure and exhibited much higher activity due to the modified band levels and band gaps.200 Ta-based oxides are known to be active photocatalysts for water splitting under UV irradiation. Under band gap (4.0 eV) irradiation, Ta2O5 alone can only produce a very small amount of H2 and no O2 from pure water.157,182 After modification with NiO and RuO2 as the cocatalysts, it displayed great activity for the overall water decomposition.201 The addition of Na2CO3 is also effective for improving the photocatalytic activity of Ta2O5, as observed for the TiO2 photocatalytic system.78 Mesoporous Ta2O5 was found by Domen and co-workers to be an active catalyst for photocatalytic water decomposition after NiO loading.202 Although the walls of the mesoporous Ta2O5 were amorphous, the photocatalytic activity was higher than that of crystallized Ta2O5. This was because the small wall thickness of mesoporous Ta2O5 favored the migration of excited electron to the surface. When mixed with TiO2, the mesoporous Ta-Ti mixed oxides formed showed relatively high activities for photocatalytic hydrogen generation from methanol/water mixtures under the irradiation of λ > 300 nm. However, a higher concentration of TiO2 in the mixed oxides led to the destruction of the mesoporous structure.203 In contrast, the introduction of MgO into the mesoporous structure of Ta2O5 improved the thermal stability and also gave rise to stable photocatalytic activity for overall water decomposition over Mg-Ta mixed oxides.204 Ni-mixed mesoporous Ta oxide possessed an incomplete mesoporous structure but exhibited higher photocatalytic activity for overall water decomposition than nonmodified mesoporous Ta oxide under UV irradiation, while Cu-mixed mesoporous Ta oxide evolved H2 only at a low rate.205 In 1998, Kato and Kudo reported that alkali tantalates ATaO3 (A ) Li, Na, and K) showed high activities for photocatalytic water splitting into H2 and O2 under UV irradiation.201 The excess of alkali in the synthetic process of the solid-state reaction improved the photocatalytic activities of naked tantalates. The order of the activities was KTaO3 , NaTaO3 < LiTaO3.206 Nickel oxide207,208 and nanosized gold particles167 were shown to function as

Chen et al.

efficient cocatalysts for photocatalytic water splitting. Among them, NiO/NaTaO3 was the most photocatalytically active and produced H2 and O2 from pure water with a quantum yield of 28% at 270 nm.207 Compared to the solid-state reaction method, both the hydrothermal method209,210 and the sol-gel method211 produced ATaO3 (A ) K, Na) with good crystallinity as well as high surface areas. These exhibited higher photocatalytic activity in water splitting than the solidstate produced material. Ishihara and co-workers found for the first time that controlling the charge density in KTaO3 by doping small amounts of acceptors such as tri- or tetravalent cations was effective for improving the photolysis activity of H2O.212,213 In particular, NiO/KTaO3 doped with 8 mol % Zr4+ exhibited a higher photocatalytic activity than the well-known photocatalyst Pt/TiO2. The increased activity was brought about by an increase in the lifetime of the photoexcited charge, which in return was caused by a decrease in the charge density. Kudo and Kato investigated the effects of doping lanthanide (La, Pr, Nd, Sm, Gd, Tb, and Dy)214 and alkalineearth metal ions (Ca, Sr, and Ba)215 into NaTaO3 photocatalysts for efficient water splitting. Lanthanum was the most effective dopant. The apparent quantum yield at 270 nm amounted to 56%,20 which is the highest quantum yield ever reported for catalysts in pure water splitting. The positive effects on the photocatalytic properties were mainly due to the decrease in the particle size and the ordered surface nanostructure. The many characteristic steps created by the doping affected the electron-hole recombination kinetics as revealed by a time-resolved infrared absorption study of the NaTaO3-based photocatalysts.216,217 The related photocatalyts NiO/A2Ta2O6 (A ) K, Na) also worked efficiently for overall water splitting under UV irradiation.218,219 For the alkalineearth tantalates ATa2O6 (A ) Ca, Sr, Ba), the order of photocatalytic activities was SrTa2O6 > BaTa2O6 > CaTa2O6. This corresponded to the band gaps and the energy of the photogenerated-electron/hole pairs transferring in the crystal (emission energy).201,208,220 When the NiO cocatalysts were loaded, NiO/SrTa2O6 showed the highest activity for overall water splitting. The quantum yield was 7% at 270 nm.220 In the related series of strontium tantalates SrmTanO(m+5n/2), the photocatalytic activities for water splitting into H2 and O2 decreased in the following order: Sr2Ta2O7 > Sr5Ta4O15 > SrTa2O6 > Sr4Ta2O9.221 The quantum yield of NiO (0.15 wt %)/Sr2Ta2O7 prepared by the polymerized complex method was estimated to be ∼24% at 270 nm.21,222 Substitution of Ta for Nb reduced the band gap of Sr2Ta2O7 from 4.5 to 3.9 eV.222,223 Under UV irradiation, all the Sr2(Ta1-xNbx)2O7 solid solutions loaded with NiO cocatalysts decomposed water into H2 and O2 stoichiometrically. But the photocatalytic activity decreased dramatically even when the amount of Nb was small. Ca2Ta2O7 with a pyrochlore structure produced H2 and O2 in a stoichiometric ratio under UV irradiation. The activity was higher than NiO-loaded niobate pyrochlore, NiO/ Ca2Nb2O7.218 Otsuka et al. claimed that, in comparison to BaTa2O6, Ba5Ta4O15 prepared under a Ta-rich atmosphere showed a higher photocatalytic activity in the decomposition of H2O into H2 and O2 under UV irradiation.224 When Ta was partially replaced by Ni or Zn, only H2 from water was evolved from the resulting BaM1/3Ta2/3O3 (M ) Ni, Zn). Methanol was the electron donor, and Pt was the cocatalyst.178,225 Shimizu and co-workers first developed A2A′Ta2O7 (A ) H, K, and Rb; A′ ) Sr and La2/3) with a hydrated layered perovskite structure. It proved highly efficient for overall


water splitting, even without cocatalysts loading.226,227 These catalysts showed higher activities than the anhydrous perovskites (Li2SrTa2O7, La1/3TaO3, and KTaO3). This was attributed to their hydrated layered structure where the photogenerated electrons and holes can be effectively transferred to the interlayer water. Moreover, as a result of the intercalation of small NiO clusters into the layers of H2La2/3Ta2O7 via an ion-exchange reaction, their cocatalyst action remarkably increased the overall activity. This was achieved by shortening the migration distance of the photogenerated charges to the reactive sites. On the other hand, the relatively large NiO particles at the external surface of H2SrTa2O7 did not improve the activity. Interestingly, hydration under aqueous conditions changed the crystal structure of K2Sr1.5Ta3O10 from orthorhombic to a tetragonal symmetry. This was due to water intercalation into the interlayer space.228 With RuOx as the cocatalyst, the hydrous K2Sr1.5Ta3O10 photocatalyst was active in the pure watersplitting process: the quantum yield at 252.5 nm was ∼2%. For the layered perovskites ACa2Ta3O10 (A ) Cs, Rb, K, Na, and Li), interlayer hydration was only observed for A ) Na and Li.229 Hydration of the Li phase doubled the rate of photocatalytic gas evolution when loaded with the cocatalyst NiO; this was the highest in the ACa2Ta3O10 series. Analogously, a quantum yield of 8% was achieved for the Ba-based (100) layered perovskite KBa2Ta3O10, after modification with NiO.134 Li et al. prepared another hydrated layered perovskite, namely, the tantalate H1.81Sr0.81Bi0.19Ta2O7, from Bi2SrTa2O9 using an ion-exchange reaction in hydrochloric acid solution.230 Under UV irradiation, the H1.81Sr0.81Bi0.19Ta2O7 photocatalyst showed favorable photocatalytic activity in splitting pure water into H2 and O2 even without the assistance of a cocatalyst. Layered lanthanide tantalates and their ion-exchanged phases (MLnTa2O7, M ) Cs, Rb, Na, and H; Ln ) La, Pr, Nd, and Sm) were prepared by Machida and co-workers to evaluate their photocatalytic activity for water splitting under UV irradiation.231-234 The photocatalytic activity was sensitive to not only Ln but also the interlayer cation, M. The highest activity was obtained for M ) Rb with the following sequence of Ln: Rb > Nd > Sm > La > Pr. The effects of lanthanide ions on the photocatalytic activities of LnTaO4 (Ln ) La, Ce, Pr, Nd, and Sm) with monoclinic structures and K2LnTa5O15 (Ln ) La, Pr, Nd, Sm, Gd, Tb, Dy, and Tm) with tungsten bronze structures were also investigated by Machida’s group.235,236 The photocatalytic activities for water splitting under UV irradiation strongly depended on the particular lanthanide ion. For the LnTaO4 series, LaTaO4 showed the highest rate for the stoichiometric evolution of H2 and O2 from pure water; while among the K2LnTa5O15 series, K2PrTa5O15 and K2SmTa5O15 showed relatively high activities for water splitting (hν > 3.9-4.1 eV). The photocatalytic activity of R3TaO7 (R ) Y, Yb, Gd, La) for water splitting was studied by Arakawa and co-workers.131,192 They examined the effect of R3+ ionic radius on the crystal structure.131,192 The crystal structures of R3TaO7 changed with increasing ionic radius of the R3+ ion from a fluorite-type cubic structure to a pyrochloretype cubic structure and finally to a weberite-type orthorhombic structure. In the case of the La3TaO7, the photocatalytic activity was greatly increased by the phase transition from cubic to orthorhombic. K3Ta3Si2O13 and K3Ta3B2O12, which have similar crystal structures, consisting of pillars formed


by a corner sharing of three linear TaO6 chains, were active for water splitting without any cocatalyst.237,238 The TaO6 pillars in K3Ta3Si2O13 and K3Ta3B2O12 are linked by Si2O7 ditetrahedral units and BO3 triangle units, respectively. Thus, the bond angle of O-Ta-O in K3Ta3B2O12 (171.5°) is slightly smaller than that in K3Ta3Si2O13 (173.1°). The distortion due to the smaller bond angle of K3Ta3B2O12 than that found in K3Ta3Si2O13 resulted in a wider band gap and higher photocatalytic activity. NiO cocatalyst loading increased the activity of K3Ta3Si2O13 drastically but proved ineffective for K3Ta3B2O12. In a manner similar to niobates, the tantalates ATaWO6 (A ) Rb, Cs) crystallized into a defect pyrochlore structure with a conduction band composed of the W5d orbital hybridized with the Ta4d orbitals.176 Under UV irradiation, they evolved H2 and O2 in a stoichiometric ratio from an aqueous AOH (A ) Rb, Cs) solution. It was loaded with NiO as cocatalyst. Even though the pyrochlore-like Bi2MTaO7 (M ) Y and La) showed a strong optical absorption in the visible region, as photocatalyts these oxides could only produce H2 and O2 from pure water under UV irradiation.239 Chen and co-workers investigated the photocatalytic water splitting of La2AlTaO7 with a view to studying the effect of aluminum on the electronic structure.240 It was found that instead of the Ta5d state it was the Al3s3p states that acted as the lower conduction band. Under UV irradiation, La2AlTaO7 showed photocatalytic activity in splitting pure water into H2 and O2 even in the absence of a cocatalyst. In comparison, using ABi2Ta2O9 (A ) Ca, Sr, Ba), also developed by Chen’s group, H2 or O2 evolved only from the aqueous solution containing either methanol or AgNO3 as the sacrificial reagent. Simultaneous production of H2 and O2 from pure water was not observed.241 The photocatalytic activities decreased in the order of SrBi2Ta2O9 > CaBi2Ta2O9 > BaBi2Ta2O9. A large range of transition-metal tantalates has been investigated by different researchers with water decomposition as the aim. Under UV irradiation, NiTa2O6 produced both H2 and O2 from pure water without a cocatalyst. On the other hand, with MnTa2O6, CoTa2O6, CrTaO4, PbTa2O6, FeTaO4, and BiTaO4, only traces of H2 evolved.200,201 When NiO was loaded as the cocatalyst, AgTaO3 and ZnTa2O6 were active in water splitting, producing both H2 and O2.201,242 In contrast, in an aqueous methanol solution, Sn2Ta2O7 with Pt as the cocatalyst only produced H2 while SnTa2O6 was totally inactive.243

3.1.3. W-, Mo-Based Oxides The number of heterogeneous photocatalysts based on either tungstates or molybdates for H2 or O2 evolution is quite small. Some were found to be active for water splitting only under UV irradiation even though they showed optical absorption in the visible region. Inoue and co-workers found that PbWO4 incorporating a WO4 tetrahedron showed high and stable photocatalytic activity for the overall splitting of water. A stoichiometric quantity of H2 and O2 was produced under UV irradiation when RuO2 was loaded onto the metal oxide.244,245 The photocatalytic performance was attributed to large dispersions in both the valence and conduction bands. This generated very mobile photoexcited holes and electrons. In contrast, a small dispersion in the conduction band was observed for the photocatalytically inactive CaWO4, which has a similar crystal structure. PbMoO4 catalyzed hydrogen evolution from aqueous methanol solution. It also was capable of oxygen evolution from aqueous silver nitrate


solution under UV irradiation, and its oxygen evolution activity was comparable to that observed on TiO2.246 Kudo and co-workers have extensively investigated the photocatalytic activities of tungstates and molybdates.247,248 Under UV irradiation, Na2W4O13247 and Bi2W2O9,145 with layered structures, were active for photocatalytic hydrogen (Pt as cocatalyst) and oxygen evolution in the presence of suitable sacrificial reagents. However, Bi2MoO6 with a similar structure evolved only oxygen from AgNO3 aqueous solution at a low rate.145 They also found that some scheelitetype molybdates and tungstates functioned as photocatalysts for both H2 or O2 evolution in the presence of sacrificial reagents.248 The band gaps (BGs) of scheelite compounds narrowed when they were composed of Ag+ and Bi3+ ions. (NaBi)0.5MoO4 (BG ) 3.1 eV), (AgBi)0.5WO4 (BG ) 3.2 eV), and (AgBi)0.5MoO4 (BG ) 3.0 eV) all showed photocatalytic activity for O2 evolution from an aqueous solution containing an electron acceptor. On the other hand, (NaBi)0.5WO4 (BG ) 3.5 eV) produced H2 from an aqueous solution containing an electron donor. In comparison, (AgLn)0.5MoO4 (Ln ) La, Ce, Eu, Yb) barely produced H2 or O2 from aqueous solutions under UV irradiation. Nguyen et al. developed a novel silicotungstic acid (SWA)-SiO2 photocatalyst by impregnating of SWA on a silica support.249 Under UV irradiation, an approximately stoichiometric production ratio of H2 and O2 was observed on these SWA-SiO2 photocatalyts. The role of the photoactive sites in SiO2 as a donor source for hydrogen formation and that of SWA as an inhibitor for the recombination of photoexcited electrons and holes were appreciable and responsible for the superior photocatalytic performance of the SWA-SiO2 system.

3.1.4. Other d0 Metal Oxides Some other miscellaneous d0 metal oxides that can catalyze water splitting to H2 and/or O2 under UV irradiation are described below. Wang et al. observed that a new crystal structure for nanostructured VO2, with a body centered-cubic structure (bcc) and a large optical band gap of ∼2.7 eV, surprisingly showed excellent photocatalytic activity in hydrogen production from a solution of water and ethanol under UV irradiation.250 The bcc VO2 phase exhibited a high quantum efficiency of ∼38.7% when synthesized as nanorods. Luan and co-workers first prepared Bi2GaVO7 and Bi2YVO8 with tetragonal structures by solid-state reactions. These two compounds initiated both H2 and O2 evolution from pure water only under UV irradiation. This is in spite of the fact that both of them showed strong optical absorption in the visible region (λ > 420 nm).251,252

3.2. d10 Metal Oxide Photocatalyts Various typical metal oxides with d10 (In3+, Ga3+, Ge4+, Sn4+, Sb5+) configurations have all been shown to be effective photochemical water-splitting catalysts under UV irradiation. Of these, Ni-loaded Ga2O3 was one of the promising photocatalysts for overall water splitting.253 Its photocatalytic activity could be effectively improved by the addition of Ca, Cr, Zn, Sr, Ba, and Ta ions.254 In particular, Zn ion doping remarkably improved the photocatalytic activity, with an apparent quantum yield for Ni/Zn-Ga2O3 of ∼20%. By combining with Lu2O3, the resulting Zn-doped Lu2O3/Ga2O3 proved to be a novel composite photocatalyst for stoichiometric water splitting under UV irradiation. When

Chen et al.

the system was loaded with NiO as the cocatalyst, the quantum yield at 320 nm was estimated to be 6.81%.255 For solid solutions consisting of Ga2O3 and In2O3, Ga1.14In0.86O3 showed the highest photocatalytic activity for H2 evolution from aqueous methanol solutions and for O2 evolution from aqueous silver nitrate solutions.256 In comparison, the solid solutions of Y2O3 and In2O3, Y1.3In0.7O3, showed the highest photocatalytic activity for the overall water splitting when combined with RuO2 as a promoter.257 Inoue and co-workers investigated the photocatalytic properties for water decomposition of alkali metal, alkaline earth metal, and lanthanum indates with an octahedrally coordinated In3+ d10 configuration ion.258-262 The photocatalytic activity for water decomposition under UV irradiation was considerably large for RuO2-dispersed CaIn2O4, SrIn2O4, and Sr0.93Ba0.07In2O4 but very poor for RuO2-dispersed AInO2 (A ) Li, Na) and LnInO3 (Ln ) La, Nd). The geometric structures of the InO6 octahedral units for these indates were compared. It was shown that the photocatalytically active indates possessed distorted InO6 octahedra with dipole moments. The internal fields that arose because of the dipole moment promoted the charge separation in the very initial process of photoexcitation. In addition, the broad sp conduction bands with large dispersions permitted the photoexcited electrons to move to the dispersed promoter RuO2 particles. A group of p-block metal oxides was reported to have stable activity in decomposing water to H2 and O2 under UV irradiation when combined with RuO2 or Pt as cocatalyt.261-268 They consist of metal ions with d10 configurations and have distorted octahedral and/or tetrahedral structures. For example, the distorted SbO6 octahedra in M2Sb2O7 (M ) Ca, Sr),263 CaSb2O6,263 and NaSbO3,263 the distorted GeO4 tetrahedra in Zn2GeO4,265 and the distorted InO6 octahedra and GeO4 tetrahedra in LiInGeO4266 were dominantly responsible for photocatalytic activity for water decomposition. Some other metal oxides with d10 configuration such as ZnGaO4,264 Sr2SnO4,261 and SrSnO3267,268 were also reported to show photocatalytic activity for water splitting.

3.3. f0 Metal Oxide Photocatalysts The f-block metal oxides usually combined with other metal oxides as photocatalysts. Pure CeO2 powder was reported to show a consistent activity toward O2 production in aqueous solutions containing Fe3+ and Ce4+ as electron acceptors.269 Sr2+-doped CeO2 was an active photocatalyst for overall water splitting when RuO2 was loaded as a promoter.270 Ce(III) oxide supported zeolites showed higher photocatalytic activity for pure water splitting.271 Nonstoichiometric H2 and O2 evolution was observed. Photoirradiation of Ce3+ species generated electrons (Ce3+ + hν f Ce4+ + e-) that were captured effectively by a water molecule for the production of hydrogen. Yuan et al. reported that BaCeO3 produced H2 and O2 from aqueous solutions containing CH3OH and AgNO3 sacrificial reagents, respectively. It also showed some activity under UV irradiation for overall water splitting with the aid of RuO2 loading.272

3.4. Nonoxide Photocatalysts More than 25 years ago, efficient hydrogen production was achieved by irradiating suspensions of ZnS in SO32- solutions under UV irradiation. The quantum yield was determined to be 90% at 313 nm. This was even without any noble metal as cocatalyst.273 InP, the sole phosphide photocatalyst


developed so far, can also produce H2 from water containing inorganic sacrificial reducing agents.274 Aqueous sulfite solutions are particularly efficient. For the past few years, there have been a few reports on nonoxide photocatalyts capable of decomposing pure water into H2 and O2 under UV irradiation. Maeda et al. found that the photocatalytic water-splitting activity of GaN is strongly dependent on the crystallinity of the material and the cocatalyst employed.275 Modification of well-crystallized GaN with Rh2-yCryO3 nanoparticles as a cocatalyst for H2 evolution resulted in the stable stoichiometric decomposition of H2O into H2 and O2 under UV irradiation. RuO2 modification, on the other hand, did not bring about appreciable H2 and O2 evolution. However, Zn2+, Mg2+, and Be2+ doping of GaN converted it into a remarkably active and stable photocatalyst.276 Again, the presence of RuO2 as a cocatalyst was required.276 β-Ge3N4 was another effective nitride photocatalyst to show efficient activity for splitting water into hydrogen and oxygen when combined with RuO2 nanoparticles reported by Domen’s group.24,277,278 The photocatalytic activity of RuO2-loaded β-Ge3N4 was strongly dependent on the reaction conditions employed. The highest activity was obtained when the reaction was carried out in 1 M H2SO4 aqueous solution. Moreover, treatment of as-prepared β-Ge3N4 powder under high-pressure ammonia effectively increased the photocatalytic activity by up to 4 times. This was attributed to a decrease in the density of anion defects in the bulk and surface.279 The AgBr/SiO2 catalyst prepared from a Schumann emulsion showed a stable and high photocatalytic activity for H2 generation from CH3OH/H2O solution under UV irradiation. The high activity of this AgBr/SiO2 catalyst related to photogenerated Ag species, which could act as the site for H2 formation.280

4. Approaches to Modifying the Electronic Band Structure for Visible-Light Harvesting With a view to developing photocatalytic applcations using visible-light irradiation, beginning with the photocatalytic splitting of water into H2 and O2 using TiO2 under UV irradiation,18 prophase studies were also carried out on some narrow band gap semiconductors such as CdS281,282 and WO3.283-285 However, the fact that serious photocorrosion of CdS was observed in the photocatalytic reaction286-288 and that the relatively positive conduction band of WO3 proved dissatisfactory for hydrogen production284 created the major impediments for the efficient performance of these two photocatalysts for use in visible-light-driven water splitting. Some studies were carried out to improve the photocatalytic stability of CdS,288-292 whereas others used WO3 as the photoelectrode in the photoelectrochemical cell to satisfy the energy requirement for water splitting with an applied potential.293-299 To overcome these obstacles, many efforts has been made to develop new visible-light-driven photocatalysts with high water-splitting activities. These are shown in Table 2. On the basis of numerous experimental results from the past 20 years, several common approaches have been adopted in order to make photocatalysts visible-light active for water splitting into hydrogen and/or oxygen: (1) metal or/and nonmetal ions doping for band gap narrowing; (2) developing solid solutions to control the band structure; (3) dye sensitization to make UV-light-active photocatalysts harvest visible light; (4) developing novel single-phase Visactive photocatalysts through band gap engineering.


4.1. Metal and Nonmetal Doping 4.1.1. Metal Ion Doping One of the most effective ways to develop visible-lightdriven photocatalysts is to create impurity levels in the forbidden band through metal ion doping. This makes the wide band gap photocatalysts active in the visible-light region, and this approach has been known for a long time. Over the past decades, there have been numerous reports on the modification of wide band gap photocatalysts using metal ion doping to make them visible-light active. These include doped TiO2,300-303 doped SrTiO3,303,304 doped La2Ti2O7,305 and doped ZnS,306,307 among others. Figure 6 depicts the sketch of visible-light-driven photocatalysts by metal ion doping to create active photocatalysts with wide band gaps. In the forbidden band, either a donor level above the original valence band or an acceptor level below the original conduction band is created to make the photocatalysts respond to visible light. As early as 1982, Borgarello et al. found that Cr5+-doped TiO2 could produce hydrogen and oxygen via sustained water cleavage under visible-light (400-550 nm) irradiation.308 Until now, many different metal ions have been doped into TiO2 to improve the visible-light absorption and photocatalytic activities. These include ions such as V, Ni, Cr, Mo, Fe, Sn, Mn, and so on.300-314 The electronic structures of TiO2 compounds doped with the 3d transition metals (V, Cr, Mn, Fe, Co, and Ni) were analyzed by Umebayashi et al. using ab initio band calculations (Figure 7A).315 They found that the 3d metal doping created an occupied level either in the band gap or in valence band (VB) due to the t2 g state of the dopant. The charge-transfer transition between this t2 g level and the conduction band (CB) (or VB) of TiO2 contributed to the photoexcitation under visible light. Using DV-XR calculations, Nishikawa et al. demonstrated the possibility of shifing the absorption edge of titania to the sunlight region in the case of V-, Cr-, Mn-, Fe-, Co-, Ni-, or Rh-doping and then discussed the relationship between the ionic radius and the change of the band gap (Figure 7B)316 and found that, of the cations addressed, Ni3+ and V5+ reduced the band gap most effectively. Cao et al. reported that Sn4+-doped TiO2 nanoparticle films prepared by the chemical vapor deposition (CVD) method displayed a higher photocatalytic activity than pure TiO2 under both UV and visible light.317 The visible-light absorption can be assigned to an electronic transition from the valence band to the doping energy level of the Sn4+ ions. This was located 0.4 eV below the conduction band and acted as an electron acceptor level. In contrast, Klosek and Raftery demonstrated that the visible absorption in V4+-doped TiO2 was indicative of the photoexcitation from the V 3d electron donor level to the TiO2 conduction band.318 This brings in a more efficient visible-light-driven activity for ethanol photooxidation over V4+-doped TiO2 than than of pure TiO2. The visible-lightdriven photocatalytic activity of Fe3+-doped TiO2 for water splitting was also attributed to the photoexcitation of doping the donor level (i.e., Fe 3d orbitals) to the TiO2 conduction band.319-321 Anpo and co-workers prepared various metal-ion-doped TiO2 materials using advanced ion implantation.322-327 They found that the absorption band of metal-ion-implanted TiO2 (the metals used were V, Cr, Mn, Fe, and Ni) shifted smoothly toward the visible-light region. The extent of the red shift depended on the amount and type of metal ions

Sn2+/K4Nb6O17 Sn2+/KTiNbO5 Sn2+/CsTi2NbO7 Sn2+/K2Ti4O9 Sn2+/K2Ti2O5 Sn2+/Cs2Ti6O13 K0.5La0.5Ca0.75Pb0.75 Nb3O10 K0.5La0.25Bi0.25Ca0.75Pb0.75 Nb3O10 Ca2NiWO6 BaCrO4 SrCrO4 SrTiO3:Rh SrTiO3:Ir

InTaO4:Ni BiYWO6 Bi0.5Dy0.5VO4 LiCr(WO4)2 NiNb2O6 NiTa2O6 InVO4 InNbO4 InTaO4 CaCo1/3Nb2/3O3 SrCo1/3Nb2/3O3 BaCo1/3Nb2/3O3 SrTiO3:Sb/Cr SrTiO3:Ru InTaO4:Ni BiTaO4:Cu NaNbO3:Ir/Sr NaTaO3:Ir/La BixIn1-xTaO4 AgNbO3 BaCr2O4 PbBi4Ti4O15 PbBi2Nb2O9 PbTiO3 SnNb2O6 SnNbO2 In2O3(ZnO)9 H(Rb)Pb2Nb3O10

TiO2:Cr TiO2:Fe TiO2:Sb/Ni TiO2:Sb/Cr TiO2:Sb/Rh TiO2:Ru Pt-ionized TiO2 Ir-ionized TiO2 Co-ionized TiO2 TiO2:Ti3+

photocatalyst

0.3 0.5 0.5 0.5 0.3 0.3

solid-state reaction

solid-state solid-state solid-state solid-state solid-state

reaction reaction reaction reaction reaction

0.2 0.2 0.2 0.2 0.2 0.2 0.3

0.5 0.3 0.2 0.5/0.3 0.5 0.5 0.5 0.5 0.5 0.5 0.5 0.5 0.5 0.3 0.5 0.1 0.3 0.3 0.5 0.3 0.5 0.3 0.3 0.3 0.3 0.3 1 1

0.025 0.5 0.5 0.5 0.3 0.1 0.5 0.5 0.5

mass (g)

thermal hydrolysis hydrothermal method solid-state reaction solid-state reaction solid-state reaction solid-state reaction hydrothermal method hydrothermal method hydrothermal method radiofrequency magnetron sputtering deposition solid-state reaction solid-state reaction solid-state reaction polymer complex method solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction, ion-exchange solid-state reaction, ion-exchange solid-state reaction, ion-exchange solid-state reaction, ion-exchange solid-state reaction, ion-exchange solid-state reaction, ion-exchange solid-state reaction, ion-exchange solid-state reaction

synthetic method

300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe

450-W Xe

300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 450-W Xe

300-W Xe 500-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 350-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 450-W Xe 450-W Xe 450-W Xe 300-W Xe 300-W Xe 300-W Xe 500-W Xe

450-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 500-W Xe 300-W Xe 300-W Xe 300-W Xe 500-W Xe

light source pure water, HCl (pH ) 3) pure water methanol/AgNO3 methanol/AgNO3 AgNO3 FeCl3 pure water pure water pure water methanol/AgNO3 pure water pure water pure water methanol/AgNO3 pure water pure water pure water pure water pure water pure water pure water pure water methanol/AgNO3 methanol/AgNO3 pure water methanol methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/Ce(SO4)2 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol methanol

>420 nm >420 nm >420 nm )420 nm/>420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >440 nm >420 nm >400 nm >420 nm >420 nm >420 nm >420 nm >540 nm/>420 nm >400 nm >420 nm >400 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >400 nm >400 nm >420 nm >420 nm >420 nm >440 nm >440 nm


>415 nm >400 nm >420 nm >420 nm >440 nm >440 nm >400 nm >400 nm >400 nm >420 nm

incident light

Pt/0 Pt/1.34 Pt/0.18 Pt/390 Pt/28.7

Pt/traces

Pt/115 Pt/270 Pt/90 Pt/115 Pt/25 Pt/35 Pt/traces

NiOy/33.2 RuO2/13.7 Pt-Cr2O3/18.2 Pt/2.4 ∼0.36 ∼0.4 NiOx/5 NiOx/3.5 NiOx/4.0 NiOx/1.72 NiOx/1.72 NiOx/2.74 Pt/156 Pt/5.7 33.2 RuO2/878 Pt/36.7 Pt/36.7 Pt/2.14 Pt/1.7 Pt/∼10 Pt/37.3 Pt/25.3 Pt/45.3 Pt/60 Pt/48 Pt/1.1 Pt/24

4.6 2.54 1.34 Pt/0.09

Pt-RuO2/268 3.6 0 Pt/0.12

0.7 0 0

560

20 0 0 0 0 0 413.3

16 0 24.02 123.3 7.5 1443.3 1733.3 1743.3 0 IrO2/209.3 1.3 1.1

1.8 13 16.6

NiOy/16.6 RuO2/6.3 Pt-Cr2O3/9.6 4.17

25.6 63 37 ∼21.3 2.3 1.27 0.67 0.5

Pt-RuO2/52

cocatal./O2

activity (µmol · h-1 · g-1) cocatal./H2

Semiconductor photocatalysts for water splitting under visible-light irradiation

Table 2. Visible-Light-Driven Photocatalysts for Water Splitting to Hydrogen and/or Oxygen

5.2 (420 nm)

s/8(>400 nm)

s/6(>400 nm)

5/s(420-500 nm)

0.27/21 (>400 nm) 0.95/29 (>420 nm) 0.33/28 (>400 nm)

0.66 (402 nm)

0.66 (402 nm) 0.17 (420 nm)

0.14 (435 nm)

QY (%)

664 657 657 344 344

707

711 711 711 711 711 711 707

353 559 560 660 661 661 668 668, 691 668, 691 680, 681 680, 681 680, 681 303 344 353-355 359 361 361 552 242 658 707 707, 708 707 243, 709 710 724 959

308 319 303 303 332 336 337 338 338 340

reference


synthetic method

solid-state reaction solid-state reaction sol-gel method solid-state reaction solid-state reaction citrate complex method citrate complex method solid-state reaction solid-state reaction solid-state reaction sol-gel method solid-state reaction sol-gel method sol-gel method solid-state reaction hydrothermal method solid-state reaction solid-state reaction coprecipitation method solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction Puratronic WO3 ion-exchange method solid-state reaction solid-state reaction solid-state reaction precipitation solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction solid-state reaction molten reaction molten reaction reflux method solid-state reaction reflux method solid-state reaction solid-state reaction solid-state reaction impregnation and calcination solid-state reaction solid-state reaction sol-gel method sol-gel method hydrothermal method ion-exchange method hydrothermal method

photocatalyst

SrTiO3:Mn CaTiO3:Rh CaTiO3:Cu Ca3Ti2O7:Rh BaNi1/3Nb2/3O3 La2Ti2O7:Cr La2Ti2O7:Fe K2La2Ti3O10:Fe K2La2Ti3O10:W K4Nb6O17:Ni Bi4Ti3O12:Cr NaTaO3:La/Cr K2La2Ti3O10:V K2La2Ti3O10:Zn In2TiO5:V Na(BixTa1-x)O3 CsLaSrNb2NiO9 In12NiCr2Ti10O42 Zn/Cr layered double hydroxides Na0.9La0.1Ta0.9Co0.1O3 Nd2Zr2O7 Sm2Zr2O7 K4Ce2Ta10O30 K4Ce2Nb10O30 Sm2InTaO7 Sm2InNbO7 WO3 Cs-WO3 Ca1-xBixVxMo1-xO4 Na0.5Bi1.5VMoO8 (AgNbO3)0.75(SrTiO3)0.25 BiVO4 Zn2.5VMoO8 Mg2.5VMoO8 Mg3V2O8 Zn3V2O8 CaBiVMoO8 CaBiVWO8 AgInW2O8 AgLi1/3Ti2/3O2 AgLi1/3Sn2/3O2 PbMoO4:Cr Bi2WO6 Bi2MoO6 Bi2Mo3O12 β-SnWO4 Ag3VO4 TiO2:Rh BiCu2VO6 BiZn2VO6 Ca2Fe2O5 Nb2O5:C ZnFe2O4 Ag3PO4 Li9Fe3(P2O7)3(PO4)2

Table 2. Continued

0.3 0.3 0.1 0.3 0.5 0.5 0.5 0.1 0.1 0.2 0.1 0.5 1 1 0.1 0.1 0.5 0.5 0.045 0.5 s s 0.1 0.1 1 1 0.2 0.4 0.5 0.5 0.5 1 0.5 0.5 0.5 0.5 0.5 0.5 0.5 0.2 0.2 0.5 1 0.5 0.5 0.3 0.3 0.1 0.5 0.8 0.1 0.2 0.1 0.5 0.1

mass (g)

s 500-W H 300-W Xe 300-W Xe 250-W Xe 250-W Xe 500-W H 350-W Xe 300-W Xe 300-W Xe 200-W Xe 300-W Xe 500-W Xe 500-W Xe 300-W Xe 300-W Xe 250-W Xe 250-W Xe 900-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 500-W Xe 300-W Xe 300-W Xe 150-W Xe 300-W Xe 350-W Xe 300-W Xe 350-W Xe

300-W Xe 300-W Xe 350-W Xe 300-W Xe 300-W Xe 500-W Hg 500-W Hg

light source

>400 nm >420 nm >420 nm >400 nm >420 nm 390-520 nm 390-520 nm >420 nm >420 nm >400 nm >400 nm >410 nm >420 nm >420 nm >420 nm >410 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >400 nm >420 nm >440 nm >420 nm >420 nm visible light >420 nm >420 nm >400 nm >400 nm

>440 nm >420 nm >400 nm >420 nm >420 nm >420 nm >420 nm visible light visible light 400-800 nm >400 nm >420 nm

incident light AgNO3 methanol methanol methanol methanol methanol methanol Na2S/Na2SO3 Na2S/Na2SO3 methanol methanol methanol KI KI pure water methanol methanol methanol AgNO3 methanol pure water pure water Na2SO3 Na2SO3 pure water methanol/AgNO3 AgNO3 Fe3+ AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 AgNO3 methanol AgNO3 FeCl3 + H2SO4 (pH ) 2.4) Fe3+ Fe3+ CO2/H2O methanol pure water AgNO3 KI



3.9

NiO/1565 Pt/7 17.03

Pt/1.8

Pt/8.68 0.09 0.01 NiOx/337.5 NiOx/104 NiOx/4.6 Pt/3.75

Pt/28.3 NiOx/22.7 Pt/7 Pt/0.74 Pt/30 Pt/20 ∼0.27 ∼0.06 144 58.1 Pt/4.4 RuO2/42.2 RuO2/55.5 Pt/∼50 NiO/75 Pt/0.6 Pt/16.4

cocatal./H2

1272

56.7 7.8 13 2.3

3.52 RuO2/67 490 201.4 144 324 478 ∼12.6 ∼5.4 7.2 20.4 105.9 30 7.2 165 120 143 3 110 15.2

1073.3

Pt/∼220

9

cocatal./O2


80 (480 nm)

0.14 (435 nm) 1.8 (420 nm) 0.76 (420 nm)

1.9 (420 nm) 1.3 (420 nm) 6 (420 nm)

0.23 (420 nm) 0.64 (420 nm)

19 (420 nm) 10 (420 nm) 6.3 (420 nm) 16.4 (420.4 nm) 9 (450 nm)

60.9 (410 nm)

QY (%)

344 346 347 348 178, 225 305, 349 305, 349 350 350 358 360 362 351 140 352 556 662 665, 666 667 553 154 154 714 714 715 716 284, 929 285 554 555 558 669-671 675 675 676 676 677 677 685 687 687 363 145 700 700 712 684 336 678 679 683 481 986 717 718

reference

Photocatalytic Hydrogen Generation Chemical Reviews, 2010, Vol. 110, No. 11 6521

CdIn2S4 AgIn5S8 CuInS2 CuIn5S8

CuGa2In3S8 AgGa2In3S8 AgGa0.9In0.1S2 ZnS-In2S3-Ag2S ZnS-In2S3-CuS NaInS2

AgGaS2 CuGa3S5 Ag2ZnSnS4 Cu2ZnGeS4

ZnIn2S4:Cu

Cu0.25Ag0.25In0.5ZnS2 ZnIn2S4 ZnIn2S4

Cu0.09In0.09Zn1.82S2

In2S3 AgInZn7S9

ZnS:C

ZnS:Pb/Cl

Cd0.1Zn0.9S:Ni Cd0.1Cu0.01Zn0.89S (Zn0.95Cu0.05)0.67Cd0.33S CdS-ZnS:Ag ZnS:Cu ZnS:Ni ZnS:Ni

CdS-ZnS

CdS:Ag CdS:In/Cu CdS:Mn CdS-ZnS

H2S thermal sulfurization hydrothermal method precipitation precipitation precipitation precipitation precipitation ultrasonic spray pyrolysis precipitation and heat treatment solvothermal and calcination hydrothermal method precipitation and calcination precipitation and calcination precipitation and calcination hydrothermal method surfactant-assisted hydrothermal method surfactant-assisted hydrothermal method solid-state reaction solid-state reaction precipitation and calcination precipitation and calcination solid-state reaction solid-state reaction solid-state reaction hydrothermal method hydrothermal method prepicipation and calcination hydrothermal method precipitation, calcination solvothermal method precipitation, calcination

precipitation precipitation and hydrothermal method precipitation low-temperature solutionphase synthesis precipitation hydrothermal method hydrothermal method precipitation

CdS CdS

CdS CdSe

two-step precipitation

synthetic method

CdS

photocatalyst

Table 2. Continued

0.5 0.3 0.25 0.5

450-W Xe 300-W Xe 500-W Xe 400-W Xe

300-W Xe 300-W Xe 500-W Hg 300-W Xe 300-W Xe 300-W Xe

500-W Hg 300-W Xe 300-W Xe 300-W Xe

0.1 0.05 0.3 0.3 0.3 0.3 0.1 0.015 0.01 0.7

300-W Xe

300-W Xe 300-W Xe 300-W Xe

300-W Xe

300-W Xe 300-W Xe

500-W Hg

300-W Xe

350-W Xe 350-W Xe 300-W Xe 900-W Xe 300-W Xe 300-W Xe 300-W Xe

350-W Xe

900-W Xe 300-W W-Hb 500-W Xe 300-W Hg

500-W Hg 700-W Hg

300-W Xe 300-W Xe

300-W Xe

light source

0.2

0.3 0.3 0.2

0.3

0.05 0.3

0.1

1

0.2 0.3 0.3 0.4 1 1 0.1

0.2

0.4 0.1 0.2 0.1

0.1 0.01

0.1 0.3

0.15

mass (g)

Pt/33480 Pt/2456 RuOx/1935 2007

Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + K2SO3 Na2S + K2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2SO3 Na2S + K2SO3 K2SO3 + Na2S K2SO3 + Na2S Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S+Na2SO3 Na2S + K2SO3 Na2S + K2SO3 Na2S + K2SO3 Na2S + K2SO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S+Na2SO3 Na2SO3 H2S + KOH K2SO3 + Na2S Na2S + Na2SO3 Na2SO3

>420 nm >400 nm >420 nm >420 nm >400 nm >430 nm >420 nm >430 nm >420 nm

>420 nm >420 nm >400 nm >420 nm >420 nm >420 nm >420 nm >430 nm >430 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >400 nm >400 nm >420 nm >420 nm >420 nm >420 nm

>420 nm >420 nm >400 nm

WC/∼1350 436

lactic acid Na2S + Na2SO3

>420 nm >420 nm

cocatal./H2

Na2S + Na2SO3

>420 nm

6960 Pt/200 Pt/84 Pt/∼1.4

Rh/10667 Rh/3433 Pt/3500 220 000 360 000 Pt/671.4

Pt/2960 NiS/∼2800 Ru/1607 Ru/1233

Pt/757.5

Ru/7666.7 Pt/231 Pt/562

Pt/4090

Pd/960.2 Pt/3164.7

Pt/∼90

93

Pt/585.5 1166.7 Pt/3633.3 Pt/40957.5 450 280 160

900

MoS2/5400 Pt-PdS/29 233

Pt/27333


incident light

s

cocatal./O2



QY (%)

420 nm) 1.3 (420-520 nm) 3 (500 nm)

14.2 (420 nm)

18.4 (420 nm)

7.4 (520 nm)

12.5 (420 nm)

20 (420 nm)

15.9 (420 nm) 9.2 (420 nm) 31.8 (420 nm) 37 (450 nm) 3.7 (420 nm) 1.3 (420 nm) 2.1 (430 nm)

10.2 (420 nm)

∼25 (450 nm) 26.5 (420 nm) 7 (>420 nm) 0.60 (>400 nm)

13.4 (>400 nm)

93 (420 nm)

60 (420 nm)

reference

1010 497 492, 493 492

543 543 544 545 546 500

496, 873 498 542 542

378

540, 541 375 377, 915

538

891 537

501

527

374 368 369-371 282 306 307 365

282 366 367 373, 529, 534, 535 536

786 974

281, 728, 730, 732, 927, 957 782 733


solid-state reaction solid-state reaction H2S thermal sulfurization H2S thermal sulfurization coprecipitation, calcination hydrothermal method NH3 nitridation, postcalcination

NH3 nitridation, postcalcination NH3 nitridation NH3 nitridation NH3 nitridation

NH3 NH3 NH3 NH3 NH3

La-In oxysulfide La-Ga oxysulfide La10OS14 La4In5S13 ZnS1-x-0.5yOx(OH)y ZrW2O8:S (Ga0.88Zn0.12)(N0.88O0.12)

Zn1.6GeN1.7O0.5

Sr2Nb2O7:N Y2Ta2O5N2 Zr2ON2 ZnxTiOyNz (SrTiO3)1-x · (LaTiO2N)x Ga-Zn-In mixed oxynitride CaTaO2N SrTaO2N BaTaO2N LaTaON2 Nb2Zr6O17-xNx N-doped Zn-Ga mixed oxide ZrxTa1-xO1+xN1-x TiN film TiO2:N TiO2:N TiO2:B/N TiNxOyFz TiO2:S/N TiO2:In/N Ca0.25La0.75 TiO2.25N0.75 TiSi2 graphitic C3N4 C3N4-xSx barbituric acid modified C3N4

TaON Ta3N5 LaTiO2N

300-W Xe 300-W Xe 300-W Xe 450-W Wc 400-W H 300-W Xe 300-W Xe 288-W F 300-W Xe

0.4 s 0.1 1.0 0.15 0.1 0.35 0.05 0.2 2 0.1 0.1 0.1

Alfa thermal condensation H2S thermal sulfurization copolymerization

H 300-W Xe 300-W Xe 500-W HBO

300-W Xe 300-W Xe 300-W Xe 300-W Xe 450-W Xe 125-W Hg

0.2 0.2 0.2 0.3 0.5 0.02

NH3 nitridation NH3 nitridation NH3 nitridation NH3 nitridation NH3 nitridation solid-state reaction NH3 nitridation cathodic arc technique precursor heat-treatment NH3 nitridation sol-gel method precursor nitridation thermal decomposition polyol method NH3 nitridation

450-W Hg


300-W Xe 300-W Xe 300-W Xe

450-W Hg

300-W Xe 300-W Xe 500-W Xe 500-W Xe 400-W H 300-W Hg-Xe 450-W Hg

300-W Xe


light source

0.2

0.1 0.3 0.2/0.05 0.2 0.15

0.4 0.2 0.2

0.1

0.1 0.1 0.2 0.2 0.1 0.1 0.3

0.2

0.5 0.5 0.3 0.3 0.2

mass (g)

methanol/AgNO3 methanol methanol methanol ethanol H2S+KOH methanol methanol Na2S Na2SO3 AgNO3 EDTA-2Na AgNO3 methanol methanol AgNO3

>400 nm >420 nm >420 nm >420 nm >420 nm >420 nm visible light >420 nm >400 nm >400 nm >420 nm >420 nm >420 nm >400 nm quartz filter >420 nm

pure water TEA/AgNO3 TEA TEA

methanol/AgNO3 ethanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol/AgNO3

>400 nm >420 nm >420 nm >420 nm >420 nm

310-800 nm >420 nm >420 nm >420 nm

ethanol/AgNO3 methanol/AgNO3 methanol/AgNO3

>420 nm >420 nm >420 nm

>400 nm

Na2S + Na2SO3/AgNO3 Na2S + Na2SO3/AgNO3 Na2S + Na2SO3 Na2S + Na2SO3 Na2S + Na2SO3 AgNO3 pure water + H2SO4 (pH ) 4.5) pure water

>420 nm >420 nm >500 nm >500 nm >420 nm >400 nm >400 nm

∼5 Pt/107 Pt/∼750 Pt/294

Pt/9.97 Pd/75

Pt/34.9

Ru/∼250 Pt/∼150a Pt/∼250

Pt/75 Pt/100 Pt/75 Pt-Ru/126.7 8566 Rh-Cr2O3/37202

Rh/50

Pt/93 Pt-Ru/833 Pt/7 Pt/0.4 Pt/66.7

Ru/300 Pt/∼125 Pt/∼15

Rh2-yCryO3/3160

Rh2-yCryO3/2800

Pt/∼85 Pt/1080 Ru/0.45 Pt/0.5 ∼460

Na2S + Na2SO3/AgNO3 Pt/105

>440 nm

cocatal./H2 18 2.64 Pt/∼0.5 Pt/223.3 Pt/110

Na2S Na2SO3 ethanol Na2S + Na2SO3 Na2S + Na2SO3/AgNO3


>420 nm >400 nm >420 nm >420 nm >440 nm

incident light

QY (%)

0.59 (420 nm) 0.3/0.7 (440650 nm)

3.7 (420 nm)

reference 954 956 440 528 485, 486, 488

∼2.5 RuO2/∼8.3

IrO2/500

∼420

221

CoOx/∼100

trace 467 46 400 53.3

1650 2100 51

0.1/s(420-460 nm)

0.4 (400 nm) 5 (420-600 nm)

14 (>420 nm)

13.5 (550 nm) 5.1%

2.1/34 (420-500 nm) s/10 (420-600 nm) 0.15/1.5 (420-600 nm)

719 720, 763 721 722

898 731 430, 431 708 465 460-462 463 525 475

42 42 42 394 398 483

581

399 393 396 482 562

390, 468, 469, 740 390, 470, 894 475, 476

0.1/s 488 (440-650 nm) IrO2/∼26 0.2/0.1 (420-600 nm) 489, 490 IrO2/∼10 2.5/0.2 (420-600 nm) 490 491 491 3.0 (400-700 nm) 547 ∼50 484 Rh2-yCryO3/1400 5.9 563, 564, 567, 569-571, (420-440 nm) 575, 767-770, 773 Rh2-yCryO3/1580 2.0 (420-440 nm) 577-580

120

110

cocatal./O2



NH3 nitridation

nitridation nitridation nitridation nitridation nitridation

hydrothermal method solvothermal method precursor heat-treatment hydrothermal method H2S thermal sulfurization or solid-state reaction H2S thermal sulfurization

Na14In17Cu3S35 · xH2O Cu8Ge5S164TiO2:S In(OH)3:S/Zn Sm2Ti2S2O5

Gd2Ti2S2O5

synthetic method

photocatalyst

Table 2. Continued


Cu2O/WO3

CaFe2O4/PbBi2Nb0.9W0.1O9

Cr2O3/Na2Ti2O4(OH)2

CaFe2O4/MgFe2O4 CdS/Na2Ti2O4(OH)2

Cu2O/CuMnO2 CuAlO2/TiO2 CuFeO2/SnO2 ZnFe2O4/SrTiO3 CdS/AgGaS2 TiO2/AgGaS2

(Pt,Cd0.8Zn0.2S)/HLaNb2O7 CdS/ETS-4 CdS/ETS-10 CdS/Ti-MCM-41 WS2/TiO2 CdS/Zr0.25Ti0.75PO4

(Pt,Cd0.8Zn0.2S)/HNbWO6

CdS/K2Ti3.9Nb0.1O9

Bi2S3/TiO2 CdS/ZnO CdS/LaMnO3 CdS/KNbO3 TiO2-xNx/WO3 MWNT/TiO2 c-CdS/Pt/hex-CdS CdSe/CdS HLaNb2O7/(Pt, Fe2O3)

CdS/TiO2

HTaWO6/(Pt, TiO2)

TaON/ZrO2 HTiNb(Ta)O5/Fe2O3

Cr-Ba2In2O5/Cr-In2O3 Ba2In2O5/In2O3 WO3/W/PbBi2Nb1.9Ti0.1O9

mesoporous graphitic C3N4

graphite oxide

photocatalyst

Table 2. Continued

modified Hummers’ method silica templated selfpolymerization solid-state reaction coprecipitation method solid-state reaction, chemical vapor deposition NH3 nitridation stepwise intercalation reaction stepwise intercalation reaction precipitation, solgel method hydrothermal method two-step precipitation reverse micelle method ion adsorption, precipitation sol-gel chemical vapor deposition direct deposition colloidal synthesis ion-exchange, photodeposition cation exchange, sulfurization cation exchange, sulfurization cation exchange, sulfurization ion exchange, sulfurization ion exchange, sulfurization ion exchange, sulfurization photodeposition ion exchange, thermal treatment, sulfurization ion exchange direct mixing direct mixing solid-state reaction solid-state reaction, precipitation solid-state reaction, sol-gel method polymerized complex method hydrothermal, ion exchange, sulfurization hydrothermal, impregnation route solid-state reaction, hydrothermal method electrodeposition

synthetic method

2

0.3

0.1

0.3 0.15

0.25 0.1 0.1

0.05 0.375

1 0.1 0.1 0.2 0.2 0.2

1

0.1

400-W Hg

450-W Xe

350-W Xe

450-W W 300-W Xe

500-W H 200-W W-H 600-W W 600-W W 450-W Hg 450-W Hg

100-W Hg 300-W Xe 300-W Xe 350-W Xe 350-W Xe 300-W Xe

450-W Hg

300-W Xe

600-W W 300-W Xe 300-W Xe 500-W Hg-Xe 300-W Hg 150-W H 500-W Hg-Xe 300-W Xe 100-W Hg

350-W Hg

0.1 0.2 0.1 0.2 0.05 1 0.05 0.004 1

450-W Hg

300-W Xe 500-W Hg

300-W Xe 300-W Xe 450-W Xe

500-W Hg

400-W Hg

light source

1

0.4 0.1

0.5 0.3 0.3

0.1

0.5

mass (g)

methanol/AgNO3 methanol methanol/AgNO3 methanol/AgNO3 methanol/AgNO3 methanol Na2S + Na2SO3

>420 nm >420 nm >420 nm >420 nm >420 nm >400 nm >420 nm

methanol Na2S + Na2SO3 Na2S + Na2SO3 AgNO3 pure water

>420 nm >420 nm >400 nm >420 nm >400 nm

>420 nm >420 nm

∼1.9

36.4

Pt-RuO2/82.7 Pt/2680

424 21 060 11 606 410 688 Pt/4730 Pt/4200

Na2SO3 + KOH Na2S Na2S2O3 Na2S2O3 Na2S + Na2SO3 Na2S + Na2SO3 Pyrex filter Pyrex filter Pyrex filter

∼892.8 Pt/175 Pt/133 Pt/76 Pt/890 Pt/2300 Na2S Na2S + Na2SO3 + NaOH Na2S + Na2SO3 + NaOH Na2SO3 Na2S Na2S + Na2SO3

>400 nm >420 nm >420 nm >430 nm >430 nm >430 nm

∼2678

Pt/∼731

2900 Pt/3870 375 NiOx/203.5 Pd/1005 Ni/38.1 13 360 Pt/40 000 ∼372

Pt/6400

∼670

Ru/∼675 traces

Pt/15.8 Pt/16.4 Pt/49.3

Pt/1490

Na2S

Na2S

cocatal./H2 4

>400 nm

>400 nm

>420 nm >400 nm >400 nm 380-780 nm >400 nm

TEA

>420 nm

Na2S2O3 Na2S + Na2SO3 Na2S + Na2SO3 + NaOH isopropanol Na2S + Na2SO3 methanol Na2S + Na2SO3 + NaOH methanol methanol

methanol


>400 nm

incident light

675

∼312.5 ∼110

741

0.7

cocatal./O2



QY (%)

38 (>420 nm)

10.1 43.4 (420 nm)

19.7 (>420 nm) 17.5 (>420 nm)

0.5

27.2 (420 nm)

2.6 (420 nm)

20 (450 nm)

8.8 (>400 nm) 0.45 (>400 nm)

3.2 (300-600 nm)

0.14 (>400 nm)

6.06/41 (>420 nm)

0.01

reference

867

876

855

875 852-854

868 870 871 872 873 874

845 847 847 849 850 851

843

840-842

822 797, 798 799 800, 801 817, 818 821 823 824 838

803-805, 816

827

897 839

819 820 877

952

723


Na2Ti2O4(OH)2/ Pt/Eosin-Y

TiO2/Pt(alizarine)2 TiO2/Pt/zinc porphyrins TiO2/RuO2/copper phthalocyanine TiO2/Pt-RuO2/8hydroxyquinoline 1,1′-binaphthalene-2,2′diol/Pt/TiO2 ZnO/Pt/rose bengal ZnO/Pt/rhodamine B TiO2/Pt/Eosin-Y TiO2/Rh/Eosin-Y TS-1/Pt/Eosin-Y

K0.95Ta0.92Zr0.08O3/Pt/ cyanocobalamin K0.95Ta0.92Zr0.08O3/Pt/ Cr-tetraphenylporphyrin K0.95Ta0.92Zr0.08O3/Pt/ Co-tetraphenylporphyrin TiO2/Pt/[Ru(dcbpy)2dpq]2+ TiO2/Pt-RuO2/ Ru(bpy)32+ TiO2/Pt/Ru(dcbpy)3 TiO2/Pt/tetrakis(4-carboxyphenyl)porphine TiO2/Pt/Ru(bpym)32+ TiO2/Pt/ merocyanine dye TiO2/Pt/ coumarin dye TiO2/Pt/ N3 dye mesoporous TiO2/Pt/ Ru(dcbpy)2(NCS)2 mesoporous TiO2/Pt/Ru2(bpy)4L1-PF6 mesoporous TiO2/ Pt/Ru(bpy)2(him)2-NO3 Al2O3/TiO2/ Pt/Ru(bpy)32+ guanidinium/Nafion/TiO2/ Pt/Ru(bpy)32+ Db [NiFeSe]-H/ RuP/TiO2 SnO2/Pt-RuO2/ Ru(bpy)32+ K4Nb6O17/ Pt/Ru(bpy)32+ H4Nb6O17/ Pt/Ru(bpy)2(4,4′-(PO3H2)2bpy)2+ HCa2Nb3O10/Pt/ Ru(bpy)2(4,4′-(PO3H2)2bpy)2+ K4-xHxNb6O17 · nH2O/Pt/RuL3(PF6)2

photocatalyst

Table 2. Continued

300-W Xe 200-W Hg-Xe 400-500 nm

0.005 0.005 0.005 0.1 0.02 1 0.125 0.005 0.05 0.03 0.03 0.3 0.02 0.04


solid-state reaction, ion exchange solid-state reaction, ion exchange solid-state reaction, acid exchange P25 TiO2 thermal hydrolysis

commercial anatase TiO2

Montedison TiO2-U

commercial TiO2

Commercial ZnO commercial ZnO ST-01 TiO2 P25 TiO2 hydrothermal method, chemical adsorption hydrothermal method, chemical adsorption 0.04

300-W Xe

0.08

EDTA

>420 nm

300-W W-H

500-W Xe 500-W Xe 300-W Xe 200-W H 300-W W-H

400-W Hg

450-W Xe

TEA TEA + I TEA + ITEA diethanolamine TEA TEA

>430 nm >420 nm >420 nm >460 nm >420 nm >420 nm >420 nm

-

EDTA

>435 nm

1861.2

2700 2560 1111 1185.5 850

34

8920

∼568

MV2+ + methanol

1.5

4320

2880

840

685.6

10

+ EDTA

712

∼90

1293

1020 695

310

1080

300

71.6 420

4000 134

EDTA EDTA

KI

EDTA

>420 nm

>430 nm >520 nm

EDTA

MV >420 nm

direct sunlight

500-W Xe 1000-W Xe

300-W Xe

150-W Xe

2+

TEA

Aldrich

250-W W-H

>420 nm

0.005

EDTA

adsorption method

300-W Xe

>420 nm

0.01

EDTA

adsorption method

300-W Xe

>420 nm

0.025

methanol methanol

sol-gel, adsorption method

500-W Xe 500-W Xe

>420 nm >420 nm

0.04 0.04

methanol

hydrothermal method hydrothermal method

500-W Xe

>420 nm

0.04

acetonitrile + NaI

hydrothermal method

300-W Xe

>410 nm

0.05

acetonitrile + NaI

Ishihara ST-01

300-W Xe

>410 nm

0.05

EDTA acetonitrile + NaI

Ishihara ST-01

500-W Xe 300-W Xe

>420 nm >410 nm

0.05 0.05

EDTA EDTA

TiO-5 standard sample Ishihara ST-01

300-W Xe 500-W Xe

>420 nm >420 nm

0.002 0.05

145

pure water + KOH (pH ) 11) 312.5 5360

513

pure water + KOH (pH ) 11)

pure water methyl viologen (MV2 + )

575

cocatal./H2

pure water + KOH (pH ) 11)


visible light >400 nm

P25 TiO2 TiO-5 standard sample

500-W Xe 250-W W-H 450-W Xe

0.1 0.04 0.01

500-W Xe

incident light


0.1


500-W Xe

light source

P25-TiO2 thermal hydrolysis

0.1

mass (g)


synthetic method

45

257

284

cocatal./O2


Dye-sensitized semiconductor photocatalysts for water splitting under visible-light irradiation

QY (%)

14.97 (>420 nm)

10 (520 nm) 10.27 (>420 nm) 9.4 (>420 nm)

0.02 (450 nm)

0.0034 (457.9 nm)

0.5 (500 nm)

0.3 (400-500 nm)

22 (450 nm)

26 (450 nm)

10.5 (450 nm)

2.4 (350 nm)

6.7 (>420 nm)

4.5 (517 nm)

2.5 (440 nm)

1.8 (517 nm)

∼0.1 (500-650 nm)

0.06

12.2 (300 nm)

reference

649

645 645 646 647, 648, 650 651

641

639

632

627 630

625, 626

623, 624

623

604

619

618

617

616

614, 615 614, 615

614, 615

613, 642-644

613, 642-644

610 613, 642-644

609 610

611 70, 592, 605-607

633

633

633


a

2730 ∼62.5 ethanol glycerol 400-W W 300-W H 0.075 0.05 impregnation method photocatalytic reduction

visible light >420 nm

2750 716.7 3060 TEA TEA TEA 400-W H 300-W W-H 300-W W-H 0.1 0.06 0.04

>420 nm >420 nm >420 nm

4060 TEA 300-W W-H 0.02

>420 nm

4690 TEA >420 nm 300-W W-H 0.02

titanic acid short nanotubes/ Pt/Eosin-Y titanic acid long nanotubes/ Pt/Eosin-Y titanic acid nanorods/Pt/ Eosin-Y TiO2/Pt/Fe3+-Eosin-Y silica gel/Pt/Eosin-Y multiwalled carbon nanotube/ Pt/Eosin-Y Co-HPA/Pt/TiO2 Wells-Dawson heteropoly blue/ Pt/TiO2

The unit of H2/O2 evolution rate is µmol · h-1, as the weight of photocatalyst has not been given in the reference. b Tungsten-halogen lamp. c Tungsten-arc lamp.

634, 635 637, 638 20.0 (670 nm)

654 655 656 19.1 (>420 nm) 10.4 (>420 nm) 12.14 (>420 nm)

653 15.04 (>420 nm)

653 17.36 (>420 nm)

652

653 6.65 (>420 nm) 1800 TEA 300-W W-H 0.02

>420 nm

1027.5 TEA >420 nm 300-W W-H 0.04

cocatal./H2

cocatal./O2

QY (%)

Chen et al.

hydrothermal method, chemical adsorption hydrothermal method, chemical adsorption hydrothermal method, chemical adsorption hydrothermal method, chemical adsorption chemical adsoprtion chemical adsorption refluxing treatment Ti-MCM-41/Pt/Eosin-Y

aqueous reaction solution incident light light source mass (g) synthetic method photocatalyst


Dye-sensitized semiconductor photocatalysts for water splitting under visible-light irradiation Table 2. Continued

12.01 (>420 nm)

reference


implanted. The absorption maximum and minimum values stayed constant. Such a shift not only allowed the metalion-implanted TiO2 to use solar irradiation more effectively but also initiated effective photocatalytic reactions, under both UV and visible-light irradiation. It was found that Pt4+and Ag+-doped TiO2 nanoparticles also exhibited improved photocatalytic activities under visible-light or UV irradiation. This was explained as follows: the doping ions in these photocatalysts not only contributed to the visible-light absorption but also served as a recombination inhibitor by trapping electrons or holes, which in return promoted the charge separation required for the photocatalytic reaction.328,329 However, in some cases, it was found that the metal-ion dopants could also serve as the recombination sites for photoinduced charges and not a recombination inhibitor. This resulted in relatively low photocatalytic activity even under UV irradiation. In 1994, Choi et al. investigated the effects of metal ion doping on the photocatalytic activity of TiO2.330 They found that the photocatalytic activity was related to the electron configuration of the dopant ion. Of the 21 metal-ion dopants studied, Fe, Mo, Ru, Os, Re, V, and Rh ion doping significantly increased the photocatalytic activity, whereas Co and Al ion doping caused detrimental effects. The nature of the metal-ion dopant in the TiO2 significantly affected the charge recombination and electron transfer rates. An electron paramagnetic resonance (EPR) study of doped TiO2 colloids showed that Fe- or V-doped TiO2 caused the growth of the Ti3+ signal. These changes were attributed to an inhibition of the hole-electron recombination by Fe3+ or V4+ dopant. On the other hand, Mo6+ dopant behaved as an irreversible electron trap.331 Kudo and co-workers reported that Ni2+-, Rh3+-, or Cr3+doped TiO2 exhibited virtually no photocatalytic activity, whereas TiO2 codoped by Ni2+, Rh3+, or Cr3+ together with Ta5+, Nb5+, or Sb5+ led to efficient O2 evolution from water.303,332-335 Reaction conditions required Ag+ as an electron acceptor and visible-light irradiation. Doping by Ni2+, Rh3+, or Cr3+ created donor levels in the forbidden band and made TiO2 responsive to visible light. The charge balance was maintained by codoping of Ta5+, Nb5+, or Sb5+, which was needed to suppress the recombination between photogenerated electrons and holes. Ohno et al. expanded the effective wavelength of TiO2 photocatalyst into the visible region by Ru doping.336 With this particular photocatalyst, the oxygen evolution reaction occurred under the irradiation of visible light at wavelengths longer than 440 nm. Iron(III) ions were used as the electron acceptor. Kahn and co-workers found that Pt-, Ir-, and Co-ionized titania nanotubes prepared by an ion-exchange method were effective photocatalysts for the production of stoichiometric hydrogen and oxygen by water splitting under visible-light irradiation.337,338 Pt, Ir, and Co ionization all reduced the band gap energy as indicated by UV-vis absorption spectra, resulting in the visible photoresponse ability. Visible-light-responsive TiO2, obtained by self (Ti3+) doping, was found to decompose water in methanol or silver nitrate solution under visible-light irradiation. The observed absorption and photocatalytic ability in the visible-light region was ascribed to the defect levels present within the band gap of these samples.339-342 Attention has also been paid to other oxide semiconductors as host photocatalysts for metal-ion doping. Cr-doped SrTi1-xCrxO3 (x ) 0.00, 0.02, 0.05, 0.10) was prepared by a solvothermal method and showed increasing photocatalytic



Figure 6. Donor level (A) and acceptor level (B) formed by metal ion doping.

Figure 7. (A) Density of states (DOS) of the metal-doped TiO2 (Ti1-xAxO2: A ) V, Cr, Mn, Fe, Co, or Ni). Gray solid lines: total DOS. Black solid lines: dopant’s DOS. The states are labeled a-j. Reprinted with permission from ref 315. Copyright 2002 Elsevier. (B) The relationship between the ionic radius and the change of the band gap (anatase). Except for some cations, the band gaps decrease with decreasing cation size. Reprinted with permission from ref 316. Copyright 1999 The Chemical Society of Japan.

activities for hydrogen production under both UV and visible light with increasing amounts of chromium. The new band gap in the visible-light range obtained by Cr doping was attributed to the band transition from the Cr 3d to the Cr 3d + Ti 3d hybrid orbital.304 Wang et al. studied the photophysical and photocatalytic properties of SrTiO3 doped with Cr cations on different sites.343 Interestingly, (Sr0.95Cr0.05)TiO3 with Cr cations (Cr3+) doped at the Sr2+ sites showed higher

photocatalytic activity of H2 evolution under visible-light irradiation than Sr(Ti0.95Cr0.05)O3 with Cr cations (mixed Cr3+ and Cr6+) doped at the Ti4+ sites. It was concluded that, because the Cr6+ cations created the potential level of the empty Cr6+ lower than that for H2 evolution and thus behaved as the trapping center for photoinduced electrons, they should be avoided in Cr-containing visible-light-driven photocatalysts intended for water splitting. Kudo and co-workers found that Mn- and Ru-doped SrTiO3 showed photocatalytic activities for O2 evolution from an aqueous silver nitrate solution.344 Ru-, Rh-, and Ir-doped SrTiO3 loaded with Pt cocatalysts produced H2 from an aqueous methanol solution under visible-light irradiation (λ > 440 nm). In particular, the Rh (1%)-doped SrTiO3 gave a quantum yield of 5.2% at 420 nm for H2 evolution. The visible-light response of Rh-doped SrTiO3 was due to the transition from the electron donor level formed by the Rh ions to the conduction band composed of Ti 3d orbitals. When SrTiO3 was codoped with Sb5+/Cr3+, Ta5+/Cr3+, or Ta5+/Ni2+, all the resulting compounds displayed efficient photocatalytic activities for hydrogen production from aqueous methanol solutions under visible-light irradiation (λ > 420 nm).303,333-345 When Ti4+ was replaced by Ni2+ or Cr3+ in SrTiO3, the results were similar to those for Sb5+/Cr3+codoped TiO2. The charge became unbalanced, and recombination centers formed. When a second metal ion such as Ta5+ or Sb5+ was codoped to compensate for the charge unbalance and suppress the formation of the recombination centers, the visible-light absorption was maintained. Miyake and co-workers346 and Chen and co-workers347 demonstrated that both Rh3+- and Cu2+-doped CaTiO3 were good candidates for visible-light-driven oxide photocatalysis for hydrogen evolution. Reaction occurred under visible-light irradiation with methanol as the electron donor. Miyake and co-workers also found that Rh3+-doped Ca3Ti2O7 was active in photocatalytic hydrogen generation under visible light.348 Moreover, it was found that Rh3+-doped Ca3Ti2O7 with a layered structure showed higher stability in air than Rh3+doped CaTiO3 with a simple perovskite structure. Lee and co-workers studied the effects of both Cr and Fe cation substituion on the photophysical and photocatalytic properties of the layered perovskite La2Ti2O7.305,349 The contribution of these dopants led to the formation of a partially filled 3d band, which served as the electron donor level in the band gap of La2Ti2O7. It also caused the excitation of electrons from this localized interband to the conduction band of La2Ti2O7 and was responsible for visible-light absorption and the H2 evolution from water under visible light. Suzuki and co-workers reported that Fe3+ and W6+ substitution for Ti4+ in K2La2Ti3O10 resulted in a small activity for hydrogen


Chen et al.

Figure 8. (A) Optical properties of the photocatalyst. The main panel shows the ultraviolet-visible diffuse reflectance spectra of In1-xNixTaO4 (x ) 0 and 0.1) at room temperature, with the inset providing an expanded view of the spectra in the wavelength region from 400 to 600 nm. (B) Photocatalytic H2 and O2 generation. Shown are the evolution of H2 and O2 from pure water using as catalyst a suspension of NiOy/In0.9Ni0.1TaO4 (solid circles, H2; open circles, O2) and RuO2/In0.9Ni0.1TaO4 (solid squares, H2; open squares, O2). Experiments were done using 0.5 g of catalyst powder suspended in 250 mL of pure water in a Pyrex glass cell under visible-light irradiation (>420 nm). Light source: 300-W Xe lamp. The gases evolved were determined by thermal conductivity detector (TCD) gas chromatograph. The measurement uncertainties were ∼0.05%. Reprinted with permission from ref 353. Copyright 2001 Nature Publishing Group.

production under visible-light irradiation.350 Under the same condition, pure K2La2Ti3O10 showed no activity. Recently, it was reported that both V-doped and Zn-doped K2La2Ti3O10 exhibited high photocatalytic activities of hydrogen production under visible light.140,351 The hybridization of either V 3d or Zn 3d and O 2p electron orbitals resulted in a new localized energy level. The catalyst was easily excited with lower energy, which in turn improved the photoactivity of K2La2Ti3O10 for water splitting. The band gap and photocatalytic activity of In2TiO5 also underwent significant changes as a result of V doping. These enabled the absorption of radiation from the entire visible region of 400-800 nm and led to the improvement of photocatalytic hydrogen production under visible light.352 It is worth mentioning that Zou and co-workers investigated the doping effects of different metal ions (Mn, Fe, Co, Ni, Cu) on the structural and photocatalytic properties of a InTaO4 photocatalyst,353-357 as shown in Figure 8. Of these, In0.9Ni0.1TaO4 showed the highest photocatalytic activity, which induced direct splitting of water into stoichiometric amounts of oxygen and hydrogen under visible-light irradiation with a quantum yield of ∼0.66% at 402 nm. The narrower band gap of Ni-doped InTaO4 was attributed to the Ni 3d donor level formed in the forbidden band.353 Ni-modified K4Nb6O10 prepared by a solid-state reaction also exhibited increased visible-light absorption and photocatalytic activity for hydrogen evolution under visible-light irradiation. This was believed to be due to the effect of the Ni2+ doping.358 Cu 3d donor level formed above the valence band of BiTaO4 by Cu2+ doping. This contributed to the increased photocatalytic activity for hydrogen evolution under visible light compared to BiTaO4.359 The strong photoabsorption and good performance of H2 evolution in the visible-light region shown by Cr3+-doped Bi4Ti3O12 was largely attributed to the occurrence of the impurity level Cr 3d in both conduction and valence bands.360 Kudo and co-workers controlled the oxidation numbers of Ir when it substituted for Nb5+ and Ta5+ ions in the B sites of a perovskite structure for NaBO3 (B ) Nb, Ta).361 Their strategy consisted of codoping of alkaline earth metal and lanthanum ions for Na+ ions at the A sites. This

contributed to maintaining the charge balance in NaBO3. The resulting NaNbO3:Ir/A (A ) Sr, Ba, and La) showed H2 or O2 evolution, whereas NaTaO3:Ir/A showed H2 evolution under visible light. Yang et al. reported that La3+/Cr3+codoped NaTaO3 showed intense visible-light absorption and H2 production in the presence of methanol under visiblelight irradiation.362 The photocatalytic activity was much higher than that of monodoped NaTaO3. A high visible-light photocatalytic activity for O2 evolution from an aqueous solution containing an electron acceptor (quantum yield of 6% at 420 nm) was found for Cr6+-doped PbMoO4. It should be noted that the formation of an electron-acceptor level of Cr 3d orbitals below conduction band as a result of the Cr6+ replacement was believed to have given rise to the absorption bands and photocatalytic activity in visible-light region.363 Although ZnS is a highly efficient photocatalyst for H2 evolution because of its high conduction band level, it is only active in the UV light region.273,364 Hence, it would be quite interesting to see if ZnS becomes visible-light responsive while maintaining its high H2 evolution activity following some modification. With this in view, a series of Cuand Ni-doped ZnS photocatalysts were prepared. The results showed high activities for H2 evolution from the aqueous solutions containing sulfite ions under visible-light irradiation (λ > 420 nm), even in the absence of a platinum cocatalyst. The visible-light response was a result of the formation of 3d donor levels by the doped Cu2+ and Ni2+ in the wide band gap of the ZnS host photocatalyst.306,307,365 In contrast to the doping modifications described previously, which focused on UV-light-active photocatalysts, some visible-light-driven photocatalysts were also modified by metal-ion doping with the aim of narrowing their band gaps in order to utilize visible light in further longer-wavelength regions to produce more efficient photocatalytic water splitting. Reber and Meier modified the visible-light active photocatalyst CdS by doping it with Ag+ in order to extend the spectral response up to 620 nm.282 A significant enhancement in the photocatalytic activity for hydrogen evolution was obtained with CdS powders containing 0.77% Ag+. Ren et al. reported two series of photocatalysts based on CdS as the base with a little of MInS2 (M ) Cu, Ag) as the dopant.366



Figure 9. (A) Diffuse reflectance spectra of Cu-doped ZnIn2S4. (B) Dependence of photocatalytic activity for H2 evolution over Cu-doped ZnIn2S4. The concentrations of Cu2+ were (a) 0.0 wt %, (b) 0.1 wt %, (c) 0.3 wt %, (d) 0.5 wt %, (e) 0.7 wt %, (f) 0.9 wt %, (g) 1.2 wt %, (h) 1.6 wt %, and (i) 2.0 wt %, respectively. Reprinted with permission from ref 378. Copyright 2008 American Chemical Society.

The resulting compounds had narrower band gaps and higher photocatalytic activities than undoped CdS. More recently, a large degree of Mn doping was discovered to be effective in improving the photocatalytic activity and stability of CdS for visible-light hydrogen production.367 In independent studies, Liu et al.368 and Xu and coworkers369-371 reported that the Cu-doped ZnxCd1-xS solidsolution photocatalyst with the absorption edge shifted to a lower energy region displayed higher water-splitting efficiency to produce hydrogen than ZnxCd1-xS, which itself had been shown to be an excellent visible-light-driven photocatalyst.372,373 Zhang et al. found Ni2+ doping also greatly improved the photocatalytic activity of ZnxCd1-xS for hydrogen production.374 For some time it has been known that ZnIn2S4 can efficiently produce hydrogen from some aqueous solutions with sulfite and sulfide ions as the electron donor under visible-light irradiation.375-377 Shen et al. hydrothermally synthesized a series of Cu-doped ZnIn2S4 photocatalysts with broader absorptions in the visible-light region than the corresponding undoped ZnIn2S4.378 As shown in Figure 9, they found that the photocatalytic activity of ZnIn2S4 was remarkably enhanced by Cu doping. The 0.5 wt % Cu-doped ZnIn2S4 photocatalyst showed the highest activity for hydrogen evolution under visible-light irradiation. The surplus doped Cu2+ ions served as the recombination sites for the photogenerated electrons and holes.379

4.1.2. Nonmetal-Ion Doping Nonmetal ion doping is another approach used to modify UV-light-active photocatalysts. It has been widely used to narrow the band gap and improve the visible-light-driven photocatalytic activity. Unlike metal-ion dopants, nonmetalion dopants are less likely to form donor levels in the forbidden band but instead shift the valence band edge upward. This results in a narrowing of band gap as indicated in Figure 10. The technology of nonmetal-ion doping has been widely used to modify some UV-light-active oxide photocatalysts, such as Ti-based oxides,380-387 Ta-based oxides,388-395 Zr-based oxides,396-398 Nb-based oxides,398-402 etc. Various nonmetal ions (such as C, N, S, etc.) were used to dope TiO2, and the products were studied for their optical and photocatalytic properties. Nonmetal-ion doped TiO2, in which the absorption spectra were red-shifted to longer wavelengths, exhibited improved photocatalytic activities

Figure 10. New valence band formation by doping of nonmetal ions.

compared to those for pure TiO2, especially in the visiblelight region.403-416 Chen and co-workers used X-ray photoelectron spectroscopy (XPS) to show that additional electronic states exist above the valence band edge of pure TiO2 for C-, N-, and S-doped TiO2 (Figure 11A).417,418 This additional electron density of states can explain the redshifted absorption of these potential photocatalysts, as observed in the “shoulder” and “tail-like” features in the UV-vis spectra (Figure 11B). Asahi et al. studied the substitutional doping of C, N, F, P, and S for O in anatase TiO2.419 Using full-potential linearized augmented plane wave (FLAPW) method, they calculated the electronic band structures of anatase TiO2 with different substitutional dopants as shown in Figure 12. They found that the substitution of N for O, which leads to the mixing of the 2p states of N with the 2p of O, was the most effective. It led to the band gap narrowing by shifting the valence band edge upward, which in return resulted in N-doped TiO2 having a much higher photocatalytic activity than pure TiO2 in the visible-light region. Chen et al. found that the ease and degree of nitrogen doping was responsible for the significant increase in photocatalytic activity observed in the TiO2 nanocolloid versus the nitrided commercial nanopowder.414 Braun et al. revealed an additional eg resonance in the valence band of TiO2 formed by nitrogen doping in the oxygen 1s NEXAFS pre-edge.420 This extra resonance was found to bear coresponsibility for the photocatalytic performance of N-doped TiO2 at visible-light wavelengths. Up until now, N-doped TiO2 has been both widely investigated and successfully prepared by many different


Chen et al.

Figure 11. VB XPS spectra (A) and diffuse reflectance spectra (B) of (a) pure TiO2, (b) C-TiO2, (c) S-TiO2, and (d) N-TiO2. Reprinted with permission from ref 418. Copyright 2008 American Chemical Society.

Figure 12. (A) Total DOSs of doped TiO2 and (B) the projected DOSs into the doped anion sites, calculated by FLAPW. The dopants F, N, C, S, and P were located at a substitutional site for an O atom in the anatase TiO2 crystal (the eight TiO2 units per cell). The results for N doping at an interstitial site (Ni-doped) and that at both substitutional and interstitial sites (Ni+s-doped) are also shown. Reprinted with permission from ref 419. Copyright 2001 AAAS.

methods. These include physical/chemical vapor deposition,421,422 the heating of titanium hydroxide and urea,423 reactive magnetron sputtering,424,425 a hydrothermal/solvothermal process,426,427 and treating TiO2 powder in a NH3 gas flow.428,429 Yuan et al. synthesized N-doped TiO2 by heating a mixture of urea and TiO2 at 350-700 °C in air.430 XPS confirmed that both the molecularly chemisorbed N2 and the substitutional N contributed to the material response to visible light. However, the substitutional N was considered the predominate factor in improving the photocatalytic activity of the water splitting under visible light. Lin et al. demonstrated that the N-doped TiO2 photocatalyst, synthesized by a two-microemulsion technique, showed favorable photocatalytic hydrogen evolution at neutral pH range in methanol/water solutions.431 Pillai and co-workers reported that the chemical modification of titanium isopropoxide using different nonmetallic chemical reagents such as urea, sulfuric acid, and trifluoroacetic acid improved both the anatase stability and the photocatalytic activity by doping with nitrogen, sulfur, and fluorine, respectively.432-434 The photocatalytic activity of S-doped TiO2 has also been studied in depth. Using different synthetic methods, anionic sulfur can be doped into TiO2 to replace the lattice oxygen or as an cation to replace the Ti ion.407,435-438 It was found that S-doped TiO2 showed different photocatalytic activities under visible light.439 In Nishijima and co-workers’ study of S-doped TiO2, a higher activity level for hydrogen evolution than for N-doped TiO2 photocatalysts under visible light was reported.440 Kahn et al. prepared C-doped TiO2 with main rutile structure by pyrolyzing Ti metal in a natural gas flame. The C-doped TiO2 possessed lower band gap

energy and displayed a much higher photoactivity in water splitting than pure TiO2 with the mixed phase of antanse and rutile.441 It was found that C-doped TiO2 nanotubes also displayed a high photoactivity for water splitting.442 The bandgap reduction and the new intragap band formation in C-doped TiO2 nanotubes extended its utilization of solar energy up to the visible to infrared region.442 To further enhance the visible-light activity, nonmetal codoping of TiO2 such as F/B-codoping,443,444 F/Ncodoping,445,446 S/F-codoping,447 F/C-codoping,448 C/N-codoping,449,450 S/N-codoping,451,452 N/Br-codoping,453 B/Ncodoping,454,455 N/Si-codoping,456 C/S-codoping,457 and P/Fcodoping458 have all been studied. Results suggested that nonmetal-codoped TiO2 compounds had significant visible photocatalytic activities due to the synergetic effect of the codoping. Luo et al. found that Cl/Br-codoped TiO2 displayed a much higher photocatalytic activity for water splitting than either Cl- or Br-doped TiO2.459 Domen and co-workers found that N/F-codoped TiO2 had high visible-light photocatalytic activity for water oxidation due to the absorption band of TiNxOyFz in the visible region.460-462 N/S-codoped TiO2 showed considerable activity in the photocatalytic water splitting, and under visible light produced H2. This was attributed to the visible-light photoexcitation of the electrons from the isolated energy levels in the band gap formed by the doped N or S to the conduction band.463 Liu et al. synthesized B/N-codoped TiO2 with high visible-light photocatalytic activity.464 They proposed that the synergistic effects of B/N codoping created visible-light absorption by N doping, and the lifetime of the photoinduced carriers was prolonged by B doping. Subsequently, Li et al. found that the visible-light-driven photocatalytic activity of B/Ncodoped TiO2 for hydrogen evolution increased greatly compared to that of N-doped TiO2.465 They believed that the codoping of boron contributed to the excellent activity of B/N-codoped TiO2, because the doped boron could act as shallow traps for electrons, which prolong the life of photoinduced electrons and holes. Recently, OCN-doped TiO2 nanoparticles were prepared for photocatalysis in the visible-light region of 380-550 nm as indicated by UV-vis absorption spetra.466 In this doped TiO2, the OCN group bonding to titanium atoms produces a weakening of its CdO double bond and a hardening of CN and NO bonds, which enables visible absorption and related photocatalytic activity.466 Similar to the case of N-doped TiO2, N-doping in Ta2O5 also caused a valence band upward shift to a higher energy level, which narrows the band gap.391,467 TaON and Ta3N5, prepared from reacting Ta2O5 with NH3, were found to be active for water splitting into hydrogen and oxygen under visible-light irradiation.390,468-472 In particular, in the presence


of the sacrificial electron acceptor (Ag+), TaON functioned as a very efficient photocatalyst for the oxidation of water into O2 (quantum yield of 34%).468 Recently, nonmetal-iondoped titanates and tantalates have also been studied for photocatalytic reduction and oxidation under visible-light irradiation. Wang and co-workers found that, in the visiblelight range and the near-ultraviolet range, N-doped and N/Scodoped SrTiO3 displayed much higher photocatalytic activities for NO elimination than pure SrTiO3.473,474 Kasahara and co-workers found that under visible-light irradiation LaTiO2N reduced H+ into H2 and oxidized H2O into O2 in the presence of a sacrificial electron donor (methanol) or acceptor (Ag+) using the band gap transition (2.1 eV).475,476 Moreover, LaTiO2N could split water without any sacrificial reagent under visible-light irradiation when used as a photoanode in the photoelectrochemical cell.477 The visiblelight absorption was attributed to the new valence band composed of O 2p orbitals for the lower-energy side and N 2p orbitals for the higher-energy side. Similarly, because of N-doping reducing the band gap energy, N-doped KTa0.92Zr0.08O3 was reported to achieve a complete splitting of water under visible-light irradiation, when Pt was loaded as a cocatalyst.478 Yamasita and co-workers prepared MTaO2N (M ) Ca, Sr, Ba) by nitriding M2Ta2O7 at 1123 K for 15 h. MTaO2N had small band gap energies (2.5-2.0 eV) and could absorb visible light at 500-630 nm via the N 2p orbitals of the upper regions of the valence bands.42,395 Under visible-light irradiation, MTaO2N reduced H+ into H2 in the presence of a sacrificial electron donor. These oxynitrides, however, did not function in the oxidation of water due to the fact that the valence band did not have sufficient overpotentials for the oxidation potential of water. Liu et al. reported Y2Ta2O5N2 as a novel photocatalyst with high activity for water splitting into hydrogen and oxygen under visible-light irradiation in the presence of appropriate sacrificial reagents.393 The smaller bandgap energy of Y2Ta2O5N2 was attributed to the partial replacement of O2by N3- in YTaO4 and the predominant population of the valence band by a hybrid orbital between N 2p and O 2p. In addition to Ti-based and Ta-based oxides as the host photocatalysts, some other oxides with wide band gaps were also modified by using nonmetal-ion doping and were found to improve visible-light-driven photocatalytic activities for water splitting. Ji et al. studied photocatalytic water splitting using nitrogen-doped Sr2Nb2O7 under visible-light irradiation.399 After nitrogen doping, the Sr2Nb2O7 band gap energy was reduced and subsequently induced photocatalytic activity for hydrogen production from methanol-water mixtures in the visible-light region. Recently, N-doped ZrO2 and In2O3, C-doped In2O3, and Nb2O5 were also reported to show enhanced photocatalytic activities for water splitting under visible-light irradiation compared to the undoped oxide hosts.396,479-481 Hisatomi et al. found that the novel spineltype d0-d10 complex oxynitride photocatalyst ZnxTiOyNz displayed photocatalytic activity for both the reduction and oxidation of water in the presence of either a sacrificial electron donor or acceptor under irradiation at visible wavelengths.482 Li et al. demonstrated for the first time the development of a simple lamellar-solid acid photocatalyst.400 N-doped HNb3O8 displyed superior visible-light-responsive photocatalytic activity in comparison to N-doped Nb2O5 and TiO2. Kanade et al. reported that N-doped Nb2Zr6O17 gave a quantum yield of 13.5% for photocatalytic hydrogen production from the decomposition of hydrogen sulfide in


KOH aqueous solution under visible-light irradiation.398 N-doped Ga-Zn mixed oxides with a band gap of 2.6 eV were capable of producing hydrogen from a methanol aqueous solution with an apparent quantum efficiency of 5.1% under visible-light illumination.483 Rh/Cr2O3 was loaded as the cocatalyst. Some other S2- substituted metal oxides have also received considerable attention as visible-light-responsive photocatalysts for water reduction and/or oxidation. For example, the absorption edge of ZrW2O8 was significantly extended to the visible-light region by S doping.484 H2 and O2 were evolved under irradiation of up to 360 and 510 nm, respectively. The visible-light sensitization was attributed to the S 3p states, which increased the width of the valence band itself and caused a decrease in the band gap energy.484 Ishikawa and co-workers were the first to report a Ti-based oxysulfide, Sm2Ti2S2O5, as a visible-light-driven photocatalyst for hydrogen or oxygen production from aqueous solutions containing a sacrificial electron donor or acceptor.485-487 It was found that the S 3p orbitals constituted the upper part of the valence band and that these orbitals made an essential contribution to the small band gap energy. Subsequently, it was proposed that the members of the series Ln2Ti2S2O5 (Ln ) Pr, Nd, Sm, Gd, Tb, Dy, Ho, and Er) would also function as visible-light-responsive photocatalysts for water splitting. The photocatalytic activity of [Pr,Nd,Er]2Ti2S2O5, containing sulfur defects and Ti as Ti3+ was lower than that of the other Ln2Ti2S2O5 forms. It appeared that the electronic band structure was strongly affected by the lanthanoid ions.488 Recently, a number of La-based oxysulfides were shown to catalyze H+ reduction to form H2 and/or water oxidation to form O2 under visible irradiation in the presence of a sacrificial electron donor (methanol, Na2S-Na2SO3) and acceptor (Ag+), respectively. The valence bands of these photocatalysts involved overlap of the O 2p and S 3p orbitals, where the higher-energy region mainly consisted of S 3p orbitals and the lower-energy region was mainly composed of O 2p orbitals.489-491 Thus, it was deduced that the valence bands of photocatalysts consisting of S 3p orbitals, instead of O 2p orbitals, will result in the formation of narrow band gaps. From the point of view of total substitution of O2- by S2- in oxide semiconductors, some novel ternary sulfide systems, including Zn(Cu)-In-S,375,376,492-495 AgGa(In)-S,496,497 Cu-Ga-S(Se),498,499 and Na-In-S,500 have been developed as visible-light-driven photocatalysts for hydrogen production from aqueous solution containing a sacrificial reagent, such as Na2S/Na2SO3. In follow-up studies, different modification technologies were used to improve the photocatalytic activities of these single-phase sulfides. Jang et al. were the first to obtain C-doped ZnS by the calcination of a ZnS(en)0.5 complex (en ) ethylenediamine), in which carbon interacted with Zn through Zn-C bond formation.501 The participation of C 2p orbitals in the formation of the upper valence band should be responsible for the reduced band gap and the visible-light absorption of ZnS. This was confirmed by the fact that C-doped ZnS exhibited photoactivity for hydrogen production via water splitting under visible-light irradiation.

4.1.3. Metal/Nonmetal-Ion Codoping Recently, metal/nonmetal-ion-codoped semiconductor systems have been employed as photocatalysts with the objective


of improving their photocatalytic activity under visible-light irradiation. The modification of TiO2 by codoping with metal and nonmetal ions was frequently used to improve the photocatalytic activity, especially for pollutant degradation. For instance, (Ce + C, I, N, or B),502-505 (Fe + N or C),506,507 (Bi + S, C, or N),508,509 (Ni + B or N),510,511 (La + N, I, or S),512-514 and (Eu, Ta, Mo, Pt, or W + N)515-519 codoped TiO2, without exception, exhibited enhanced visible-light photocatalytic activity compared to their undoped counterparts. SrTiO3 codoped with La and N was also reported as having greater visible-light photocatalytic activity than the unmodified SrTiO3.520-522 However, only a few studies reported metal/nonmetal ion codoped photocatalyst systems with modified conduction and valence band used for visiblelight hydrogen production from water. Gai et al. proposed to dope TiO2 using charge-compensated donor-acceptor pairs such as (N + V), (Nb + N), (Cr + C), and (Mo + C).523 Among all these systems, TiO2:(Mo + C) has the highest positive effect on photocatalytic water splitting. This is because it reduces the band gap to the ideal visible-light region. It does not, however, have much effect on the conduction band position. Using density-functional theory (DFT) calculations, Yin et al. predicted that (Mo, 2N) and (W, 2N) were the best donor-acceptor combinations in the low-alloy concentration regime whereas (Nb, N) and (Ta, N) were the best choice of donor-acceptor pairs in the highalloy concentration regime for solar-driven photoelectrochemical water-splitting.524 Sasikala et al. found codoping of TiO2 with In and N in cationic and anionic sites, respectively, resulted in the narrowing of the band gap of TiO2 compared to In or N doping alone.525 As a result, the In- and N-codoped samples exhibited enhanced absorption of visible light and improved photocatalytic activity for hydrogen production. Because of the charge-compensation effect from the donor-acceptor codoping, (N, Al)-codoped ZnO obtained by radio frequency (RF) magnetron sputtering method displayed significantly reduced band gap and enhanced photocurrents under visiblelight irradiation, when compared to ZnO and Al-doped ZnO.526 Tsuji and Kudo synthesized Pb and halogen-codoped ZnS as an active visible-light-driven photocatalyst for H2 evolution without cocatalysts.527 Pb doping was responsible for the visible-light absorption, and halogen doping suppressed the formation of nonradiative transition sites in which recombination of photogenerated electrons and holes could occur. Lei et al. synthesized sulfur-substituted and Zn-doped In(OH)3 in an aqueous solution of ethylenediamine using the hydrothermal method and investigated its photoactivity for H2 production under visible-light irradiation.528 As shown in Figure 13, the band gap of In(OH)3 was narrowed by the substitution of S2- for OH-. The valence band was composed mainly of S 3p orbitals hybridized with O 2p orbitals. Meanwhile, Zn2+ doping leveled up the conduction band consisting of In 5s5p and Zn 4s4p orbitals and provided a large thermodynamic driving force for the reduction of water to produce H2.

Chen et al.

Figure 13. Proposed band structure of In(OH)3, In(OH)ySz, and In(OH)ySz:Zn. Reprinted with permission from ref 528. Copyright 2006 Elsevier.

can be adjusted by varying the ratio of the compositions of the narrow and the wide band gap semiconductor in the solid solution. Figure 14 shows the controllable band formation by making a solid solution.

4.2.1. (Oxy)sulfide Solid Solutions CdxZn1-xS (1 < x < 1) sulfide solid solutions, formed by combining the wide band gap semiconductor ZnS and the narrow band gap semiconductor CdS, have attracted much research interest for visible-light-driven photocatalysis applications.529-533 It is known that CdxZn1-xS prepared by a coprecipitation method shows quite good photocatalytic activity for hydrogen production from aqueous solutions containing sacrificial reagents S2- and SO32- under visiblelight irradiation.534,535 Zhang et al. found that Cd1-xZnxS solid solution innovatively prepared by the thermal sulfuration of the corresponding mixed oxide precursors displayed a much higher photoactivity than that prepared by the conventional coprecipitation method.536 The Cd1-xZnxS (x ) 0.2) solid solution exhibited the highest quantum yield of 10.23% at 420 nm for hydrogen production even without a noble metal as a cocatalyst. Since 2004, Kudo et al. have focused their attentions on the development of novel photocatalysts from ZnS (wide band gap) and MInS2 (M ) Cu, Ag; narrow band gap) sulfide solid solutions.537-539 The energy structures of the solid solutions were found to be controllable by changing the composition. Taking ZnS-AgInS2 as an example, the diffuse reflectance spectra, as well as the conduction and valence

4.2. Controlling Band Structure through Solid Solutions In addition to using foreign elements for doping, forming solid solutions between wide and narrow band gap semiconductors is another promising method for controlling photocatalyst band structure. Both the band gap and position

Figure 14. Band structure controlled by making a solid solution.



Figure 15. (A) Diffuse reflection spectra of (AgIn)xZn2(1-x)S2 solid solutions; the values of x are (a) 0, (b) 0.17, (c) 0.22, (d) 0.29, (e) 0.33, (f) 0.40, (g) 0.5, and (h) 1. (B) Band structures of (AgIn)xZn2(1-x)S2 solid solutions, ZnS, and AgInS2. Reprinted with permission from ref 537. Copyright 2004 American Chemical Society.

band levels, shifted monotonically with the composition of the solid solution as shown in Figure 15.537 The solid solutions showed high photocatalytic activities for hydrogen evolution under visible-light irradiation. The apparent quantum yields of Pt-loaded (AgIn)0.22Zn1.56S2 (Eg ) 2.33 eV) and Pt-loaded (CuIn)0.09Zn1.82S2 (Eg ) 2.35 eV) amounted to 20%537 and 12.5% at 420 nm,538 respectively. Subsequently, they developed a ZnS-CuInS2-AgInS2 solid solution, which proved a highly active visible-light-driven photocatalyst. It was demonstrated that the ZnSCuInS2-AgInS2 solid solution exhibited an absorption band over a wider wavelength range and a higher photocatalytic activity for hydrogen evolution under the irradiation from a solar simulator compared to the previously reported ZnS-MInS2 (M ) Cu or Ag) solid solutions. This was probably due to its narrower band gap (Cu0.25Ag0.25In0.5ZnS2: Eg ) 1.77 eV) derived from interactions between the Cu 3d and Ag 4d orbitals involved in the valence band.540,541 Another series of novel stannite-type complex sulfide solid solutions with ZnS as the wide band gap semiconductor, AI2-Zn-AIV-S4 (AI ) Cu and Ag; AIV ) Sn and Ge) was investigated by the same group, also for photocatalytic hydrogen evolution under visible-light irradiation. Among them, Ag2ZnSnS4 was the most active, with a quantum yield of ∼3% at 500 nm. Cu2ZnGeS4 also showed a high activity and had greater stability.542 The recently reported AGa2In3S8 solid solutions formed from AGa5S8 and AIn5S8 (A ) Cu or Ag) gave relatively high quantum yields. They were active for solar H2 production from aqueous solutions containing electron donors. The apparent quantum yields of Rh(1.5 wt %)/CuGa2In3S8 and Rh(0.5 wt %)/AgGa2In3S8 were 15% at 560 and 460 nm, respectively.543 Jang et al. developed novel AgGa1-xInxS2 solid solutions as visible-light-driven photocatalysts for hydrogen evolution in the presence of an electrolyte (Na2S/Na2SO3).544 The concentration-dependent band gap tuning was achieved in AgGa1-xInxS2 (0 < x < 1), which was found to vary from 2.6 to 1.9 eV due to the participation of the In 5s5p orbitals in the formation of the lower region of the conduction band. The photocatalytic activity for hydrogen production over AgGa1-xInxS2 showed the maximum value for AgGa0.9In0.1S2. Chen and co-workers synthesized two nanoporous solid solutions, i.e., ZnS-In2S3-Ag2S545 and ZnS-In2S3-CuS,546 using a facile template-free method. Both of them showed relatively high visible-light activities for photocatalytic H2 evolution from water containing sacrificial reagents of Na2SO3 and Na2S even in the absence of cocatalysts. The quantum yields were 19.8% and 22.6% at 420 nm, respectively.545,546 Li et al.

successfully prepared a zincoxysulfide (ZnS1-x-0.5yOx (OH)y) solid solution with the valence band formed by S 3p and O 2p hybrid orbitals.547 It displayed excellent photocatalytic activity for hydrogen evolution, and even without a noble metal cocatalyst, the apparent quantum yield was ca. 3.0% under visible-light irradiation.

4.2.2. Oxide Solid Solutions The photophysical and photocatalytic properties of oxide semiconductors with similar crystal structures were also studied to explore the possibility of energy structure control using solid solutions.157,256,548-550 Kudo and Mikami reported the successive changes in absorption, photoluminescence spectra, and conduction band levels of In2O3-Ga2O3 solid solutions.256 Moreover, they found that both the band gap and conduction band level of the Sr2(Ta1-xNbx)2O7 solid solution with a layered perovskite structure could be controlled by changing the ratio of niobium to tantalum. All the Sr2(Ta1-xNbx)2O7 photocatalysts studied had band gaps larger than 3.9 eV and only exhibited photocatalytic activities for water splitting into H2 and O2 under UV irradiation.223 Meanwhile, Zou and co-workers prepared BiTa1-xNbxO4 (0 < x < 1) solid-solution photocatalysts using solid-state reactions.200,551 These produced hydrogen both from aqueous CH3OH/H2O solutions and from pure water under UV irradiation. Although none of these photocatalysts exhibited visible-light-driven activities, these studies provided some important information for developing novel visible-lightdriven photocatalysts derived from oxide solid solutions that could be used for water splitting. Luan et al. prepared BixIn1-xTaO4 (0 < x < 1) solid solutions using a solid-state reaction.552 The band gaps of the BixIn1-xTaO4 (x ) 0.2, 0.5, and 0.8) photocatalysts were estimated at about 2.86, 2.71, and 2.74 eV, respectively. It was suggested that the band structure consisted of a conduction band of mainly Ta 5d, In 5p, and In 5s orbitals, whereas the valence band was principally O 2p, Bi 6s, and Bi 6p orbitals. Under visible-light irradiation (λ > 420 nm), H2 and O2 were evolved from CH3OH and AgNO3 aqueous solutions, respectively, using the BixIn1-xTaO4 photocatalysts. Yi and Ye prepared Na1-xLaxTa1-xCoxO3 monophase solid solutions by conventional solid-state reactions.553 The Na0.9La0.1Ta0.9Co0.1O3 photocatalyst exhibited the highest performance of H2 evolution (4.34 µmol/h) under visiblelight irradiation. The photocatalytic activities of Na1-xLaxTa1-xCoxO3 series were mainly attributed to the hybridization of the Co 3d and O 2p orbitals.


Chen et al.

Figure 16. (A) Schematic band structures. Reprinted with permission from ref 569. Copyright 2005 American Chemical Society. (B) UV-visible diffuse reflectance spectra of (Ga1-xZnx)(N1-xOx). Reprinted with permission from ref 51. Copyright 2007 American Chemical Society.

Since the divalent metals in scheelite-type molybdates are easily exchangeable with other elements, Yao and Ye developed new scheelite solid-solution photocatalysts by combining the scheelite molybdates (CaMoO4 and (Na0.5Bi0.5)MoO4) with the narrow band gap semiconductor BiVO4.554,555 These crystallized with similar crystal structures. Both the resulting CaMoO4-BiVO4 and (Na0.5Bi0.5)MoO4-BiVO4 solid solutions showed high activities for photocatalytic O2 evolution under visible-light irradiation. In fact, they were even better than that of monoclinic BiVO4, which itself is a well-known efficient visible-light-driven photocatalyst. In the study of Li et al., another series of novel solid-solution photocatalysts Na(BixTa1-x)O3 were successfully prepared using a simple hydrothermal method, and Na(Bi0.08Ta0.92)O3 showed the highest photocatalytic activity for hydrogen production under visible light.556 This was attributed to the band structure formed by a hybrid conduction band of the (Bi 6s + 6p + Ta 5d) orbitals. Wang et al. developed a novel series of solid-solution semiconductors (AgNbO3)1-x(SrTiO3)x (0 < x < 1) as visiblelight-active photocatalysts for efficient O2 evolution and decomposition of organic pollutants.557,558 The modulation of the band structure (band gap energy, band edge positions, etc.) depends on the extent of the orbital hybridization between both the Ag 4d and O 2p orbitals, as well as that between the Nb 4d and Ti 3d orbitals. As a result of competition between the absorption ability to visible light and the reductive/oxidative abilities, the highest visible-light activities for both O2 evolution and decomposition of gaseous 2-propanol were realized over (AgNbO3)0.75(SrTiO3)0.25. The solid solution of Y2WO6 and Bi2WO6, BiYWO6, was found by Liu et al. to have the photocatalytic ability to completely and stoichiometrically split water into H2 and O2 ratio under visible light up to λ < 470 nm.559 It was suggested that the Bi 6s and Y 4d orbitals contributed to a new valence band and conduction band, respectively. It was expected that, because of the flexible structure of the solid solution, the activity would be favorably promoted by changing the ratio of Y2WO6 and Bi2WO6. Soon after, they discovered another Bi0.5Dy0.5VO4 solid solution composed of BiVO4 and DyVO4 that responded to visible light up to 450 nm and completely split water into H2 and O2.560

4.2.3. Oxynitride Solid Solutions Starting from the colored oxynitride LaTiO2N, new perovskite-type solid solutions LaTiO2N-ATiO3 (A ) Sr, Ba) were prepared by the thermal ammonolysis method.561,562 Narrowed band gaps were achieved by both lowering the bottom of the conduction band and raising the top of the valence band as x increased. Thus, (SrTiO3)1-x · (LaTiO2N)x

presented suitable band positions for photocatalytic water splitting into hydrogen and oxygen under visible-light irradiation. Since 2005, Domen’s group has systematically investigated on GaN-ZnO solid solutions as potentially new efficient photocatalysts capable of decomposing water into hydrogen and oxygen stoichiometrically under visible-light irradiation.563-572 The solid solution of GaN and ZnO, (Ga1-xZnx)(N1-xOx), should have band gaps greater than 3 eV, because of the large band gap energies of both GaN and ZnO (>3 eV). However, the p-d repulsion between the N 2p and Zn 3d orbitals shifted the valence-band maximum upward without affecting the conduction-band minimum. This resulted in a narrowing of the band gap of GaN-ZnO solid solution as schematically depicted in Figure 16.569,573 The result, therefore, was that the band positions of (Ga1-xZnx)(N1-xOx) were suitable for overall water splitting under visible-light irradiation. The quantum efficiency at 420-440 nm was ∼2.5%, when Rh2-yCryO3 was loaded as a cocatalyst.564 The photocatalytic performance of Rh2-yCryO3/ (Ga1-xZnx)(N1-xOx) was due to the fact that the charge recombination was prevented, and there was enhanced reactivity of photoexcited holes in the O2 evolution reaction.574 Moreover, the visible-light-driven photocatalytic activity of Rh2-yCryO3/(Ga1-xZnx)(N1-xOx) was further improved by a postcalcination treatment through reduction of the density of the zinc- and/or oxygen-related defects that functioned as recombination centers for photogenerated electrons and holes in the material. The maximum quantum efficiency obtained by postcalcination treatment is ca. 5.9% at 420-440 nm.575 This was about an order of magnitude higher than the photocatalytic activity of previously discussed photocatalysts used in overall water splitting under visible light (Ni-InTaO4: 0.66% at 402 nm;353 BiYWO6: 0.17% at 420 nm559). In addition, an appropriate amount of electrolyte (e.g., NaCl and Na2SO4) in the photocatalytic reactant solution proved quite effective in enhancing overall water splitting using Rh2-yCryO3-loaded (Ga1-xZnx)(N1-xOx).576 Following the development of the (Ga1-xZnx)(N1-xOx) solid solution, (Zn1+xGe)(N2Ox),577-580 the solid solution of ZnGeN2 and ZnO was developed by Domen’s group and found to be another active and stable photocatalyst for overall water splitting under visible-light irradiation. Similar to the (Ga1-xZnx)(N1-xOx) solid solution, the band gap narrowing of (Zn1+xGe)(N2Ox) was also attributed to the p-d repulsion between the N 2p and Zn 3d orbitals. Thus, the visible-lightdriven overall water splitting catalyzed by (Zn1+xGe)(N2Ox) proceeded via band gap photoexcitation from the valence band formed by the N 2p, O 2p, and Zn 3d orbitals to the conduction band consisting of Ge 4s and 4p hybridized


orbitals. Instead of the successful formation of the ideal solid solution between (Ga1-xZnx)(N1-xOx) and InN, the obtained Ga-Zn-In mixed oxynitride also behaved as a visible-lightdriven photocatalyst for water splitting, but it photocatalyzed H2 and O2 evolution only in the presence of an appropriate electron donor or acceptor.581

4.3. Dye Sensitization to Harvest Visible Light Dye sensitization is another powerful strategy to enable the visible-light harvesting of wide band gap semiconductors.582-584 It has been actively studied in solar energy conversion systems involving dye-sensitized solar cells585-591 and dye-sensitized photocatalytic reactions.592-595 Since the breakthrough work by O’Regan and Gra¨tzel in 1991,596 the dye-sensitized solar cell has attracted much attention, owing to its stability, low cost, and device efficiency. Powerconversion efficiencies of >11% have been achieved.597-600 The operating principle of dye-sensitizated solar cells usually involves the excitation of the dye and then charge transfer from the dye to the semiconductor.601 In addition, the application of dye-sensitized solar cells to water splitting has also been achieved.602 Since the electron-transfer step resembles that in dye-sensitized solar cells, dye-sensitized semiconductors could also function as photocatalysts for water splitting under visible-light irradiation. Figure 17 illustrates the basic principle of dye-sensitized photocatalytic H2 production from water. Photoexcitation of the dye adsorbed onto the semiconductor leads to the injection of electrons into the conduction band of the semiconductor. The electrons are consumed by the reduction of water to produce H2. The oxidized dye molecules are subsequently reduced and then regenerated by accepting electrons from the electron donor.603,604

4.3.1. Sensitization Using Ruthenium Complex Dyes Photocatalytic hydrogen production systems in which ruthenium(II) complex dyes sensitize wide band gap semiconductors to visible light have been the focus of intensive research for many years. In the early 1980s, Gra¨tzel and co-workers70,592,605-607 succeeded in decomposing water by visible light using Ru(bpy)32+ and its amphiphilic derivatives as sensitizers. Pt/RuO2-loaded TiO2 particles proved particularly effective in those systems, acting as photocatalysts for water-splitting process. Nakahira et al. found that Pt/TiO2 sensitized with a polymer-pendant Ru(bpy)32+ complex was effective in H2 evolution in the presence of the sacrificial donor (EDTA) under visible-light irradiation.608 Adsorption of the Ru(dcbpy)3 sensitizer onto platinized TiO2 particles (Pt/TiO2) also

Figure 17. Basic principle of dye-sensitized photocatalytic H2 production from water. Reprinted with permission from ref 604. Copyright 2008 American Chemical Society.


led to H2 evolution by visible light, again with a sacrificial donor.609 Hirano et al. found that, when Ru(bpym)32+ was used as the visible-light sensitizer, Pt/TiO2 showed much higher efficiency for H2 production than Ru(bpy)32+.610 This may be due to the greater affinity of Ru(bpym)32+ on the TiO2 surface. Dhanalakshmi et al. found that, when TiO2 and ZnO were sensitized with a new sensitizer ([Ru(dcbpy)2(dpq)]2+), they displayed extremely stable and effcient photocatalytic activity for hydrogen production under visible-light irradiation from water even in the absence of an electron donor.611 However, interestingly, the photocatalytic activities of [Ru(dcbpy)2(dpq)]2+-sensitized Pt/ZnO and Cu/ZnO were found to be 10 times lower than those of [Ru(dcbpy)2(dpq)]2+-sensitized Pt/TiO2 and Cu/TiO2, respectviely. Bae et al. compared the photocatalytic activities and stabilities of two Ru(bpy)32+-sensitized TiO2 photocatalysts with different surface-anchoring groups (carboxylate and phosphonate), i.e., c-Ru(bpy)32+ and p-Ru(bpy)32+, respectively. Pt/TiO2/p-Ru(bpy)32+ anchored through phosphonate groups exhibited higher photocatalytic activity for hydrogen production from water than Pt/TiO2/c-Ru(bpy)32+ anchored through carboxylate groups.612 Because of the more rapid regeneration of p-Ru(bpy)32+ than c-Ru(bpy)32+, the phosphonate group seemed to be better than the carboxylate group as a ruthenium sensitizer linkage to the TiO2 surface in aqueous environment. However, both of them turned out to be unstable in water, not only under visible-light illumination but also in the dark. Abe et al. studied the effect of the energy gap between the I3-/I- redox potential and the highest occupied molecular orbital (HOMO) level of the dyes on the photocatalytic activity of Ru complex dye-sensitized Pt/TiO2 in wateracetonitrile solutions.613 The system included I- as an electron donor. It was found that a sufficiently positive HOMO level, compared to the oxidation potential of I-, was necessary in order to produce a relatively high rate of H2 evolution over Ru complex dye-sensitized Pt/TiO2. Peng and co-workers investigated the influence of different ruthenium(II) bipyridyl complexes on the photocatalytic H2 evolution over TiO2 under visible light.614,615 When compared to Ru(bpy)2(him)2-NO3- and Ru(dcbpy)2(NCS)2-sensitized Pt/TiO2, Ru2(bpy)4L1-PF6-sensitized Pt/TiO2 displayed higher photocatalytic efficiency and preferable durability for H2 evolution. This may be related to the dynamic equilibrium between the linkage of the ground dye to TiO2 and the separation of the oxidized dye from TiO2. Choi and coworkers investigated the addition of a thin Al2O3 overlayer on the Ru(bpy)32+-sensitized TiO2 and found that it significantly increased the visible-light-sensitized activity for hydrogen production.616 As shown in Figure 18, it was proven that the main role of the Al2O3 barrier layer was to retard the charge recombination between the electron injected from the excited dye and the oxidized dye. They also found that guanidinium cations adsorbed on nafion-coated Ru(bpy)32+sensitized TiO2 retarded the charge recombination between the electrons injected into the TiO2 conduction band and the oxidized dye molecules. This resulted in enhanced photocatalytic hydrogen production under visible light.617 Reisner et al. constructed a special system consisting of [NiFeSe]-hydrogenase attached to Ru dye-sensitized TiO2, with triethanolamine (TEA) as the sacrificial electron donor.618 It showed a high and stable photocatalytic activity for hydrogen generation under visible light. Gurunathan et al. found that the photocatalytic efficiency of SnO2 could be


Figure 18. Schematic illustration of electron transfer/recombination processes occurring on a dye-sensitized TiO2 particle with Al2O3 overlayer for H2 production. The numbered paths indicate the following: (1) dye excitation; (2) electron injection from the excited dye to TiO2 CB; (3) electron trapping on Pt; (4) regeneration of the oxidized dye by electron donor (D); and (5) back electron transfer to the oxidized dye (recombination). Reprinted with permission from ref 616. Copyright 2009 American Chemical Society.

greatly improved using Ru(bpy)32+ sensitization.619 The highest photocatalytic activity for hydrogen evolution, with quantum yield of 2.40% at 350 nm, was observed with the Pt/SnO2/RuO2-Ru(bpy)32+-MV2+-EDTA system. This may be due to a number of contributing factors, which include the loading of the bifunctional redox catalyst onto SnO2, electron injection from the excited Ru(bpy)32+ to the conduction band of SnO2, electron mediation by MV2+, and electron donation by EDTA to scavenge the valence band holes. Furube et al. investigated the dynamics of photoexcited Ru(bpy)32+ intercalated into the K4Nb6O17 interlayers.620 Because of the fast and efficient electron transfer between Ru(bpy)32+ and K4Nb6O17, the transient bleaching of the Ru(bpy)32+ band showed fast and nonexponential decay. This differed from the behavior of Ru(bpy)32+ in water, and led to the photocatalytic hydrogen evolution over Ru(bpy)32+ intercalated K4Nb6O17 from aqueous solution containing an electron donor.621 Later, Mallouk and co-workers studied different layered oxide semiconductors as the building blocks for visible-light H2 production from water using a ruthenium complex as the photosensitizer.604,622-626 The Ru(bpy)32+sensitized K4Nb6O17 nanoscrolls exhibited higher photocatalytic activity than Ru(bpy)32+-sensitized lamellar K4Nb6O17 and TiO2. This was primarily due to the high surface area of the nanoscrolls and their excellent ability to bind Ru(bpy)32+. This led to the facile transfer of electrons from the sensitizer to the Pt catalyst islands via the single-crystalline nanoscrolls. The authors claimed that the platinized H4Nb6O17 nanoscrolls were a slightly better electron transfer mediator than acid-restacked HCa2Nb3O10 nanosheets. The apparent quantum yield of visible-light photocatalytic hydrogen production over Pt/H4Nb6O17 nanoscrolls was ∼25% at 450 ( 20 nm, when sensitized by Ru(bpy)32+ complexes.623,624

4.3.2. Sensitization Using Other Transition-Metal Complex Dyes Many other transition-metal complexes such as polypyridine complexes, alizarine, phthalocyanine, and metalloporphyrins with metal centers including Pt(II), Co(II), Zn(II), and Cr(III) have also been widely used as sensitizers for wide band gap photocatalysts to improve their optical and photocatalytic properties for hydrogen evolution in the visiblelight region.

Chen et al.

In the study of Zakharenko et al.,627 the Pt(alizarine)2 complex adsorbed onto the surface of titanium dioxide was found to cause spectral sensitization of TiO2 and lead to photocatalytic hydrogen production from water in the visiblelight region. Two new platinum(II) terpyridyl acetylide complexes were synthesized and used by Jarosz et al.628 They were used to sensitize platinized TiO2 for the photogeneration of H2 using visible light. However, the long-term ability of these complexes to act as sensitizers in this capacity was limited by decomposition after oxidation. Malinka and co-workers found that H2 evolved from aqueous suspensions of zinc-porphyrin-sensitized Pt/TiO2 in the presence of an electron donor, such as EDTA, TEA, and ascorbic and oxalic acids, under irradiation with visible light (λ > 520 nm).629,630 Zinc porphyrins displayed increased photostability when absorbed onto the semiconductor surface, and the photocatalytic activity of zinc-porphyrin-sensitized Pt/TiO2 was greatly affected by factors such as concentrations of platinum, sensitizer and electron donor, the pH and temperature of the suspension. Shimidzu et al. found that the visible-light illumination (500 < λ < 700 nm) of a watersoluble porphyrin-zinc complex and TEA in aqueous solution with suspended particulate ZnO/Pt resulted in efficient hydrogen production with a quantum yield higher than 3.0% at 548 ( 3 nm.631 Nada et al. found that, when copper phthalocyanine was used as a photosensitizer, it was effective for hydrogen production over RuO2/TiO2 using UV/solar light irradiation.632 In fact, copper phthalocyanine exhibited higher efficiency compared to other sensitizers such as ruthenium bipyridyl. Since the splitting of pure water using a dyesensitized oxide semiconductor has not been achieved previously, it is worth mentioning that Hagiwara et al. were the first to report the sensitizing effects of porphyrinoids on the photocatalytic splitting of H2O into H2 and O2 by Pt/ KTa(Zr)O3.633 The addition of porphyrinoids to KTa(Zr)O3 effectively increased the activity of this compound for pure water splitting. Among the porphyrinoids examined, cyanocobalamin showed the strongest effect on photocatalytic water splitting. Moreover, the metal cation of the porphyrin complex had a large influence on the production rates of H2 and O2. For example, Pt/KTa(Zr)O3 sensitized with Crtetraphenylporphyrin showed much higher photoactivity than a catalyst sensitized with Co-tetraphenylporphyrin. Rayalu and co-workers reported that, because of the synergistic effect of Co2+ and heteropolyacid (HPA), HPA/ Co2+ sensitized TiO2 showed excellent photocatalytic activity for hydrogen evolution under visible light.634-636 The presence of Co2+ not only enhanced the visible-light absorption property but also played a very important role in triggering the overall catalytic efficiency. Recently, a TiO2 photocatalyst sensitized by grafting surface complexes of lacunary Wells-Dawson W-contained heteropoly blue (HPB) exhibited 20.0% quantum efficiency for H2 evolution under 670 nm irradiation in the presence of glycerol as the electron donor.637,638

4.3.3. Sensitization Using Metal-Free Dyes Because some transition-metal complexes, especially Ru complexes, are quite expensive, metal-free dyes, such as porphine dyes, xanthene dyes, melocyanine dyes, and coumarin dyes, have all been investigated. Houlding and Gra¨tzel reported the excellent ability of 8-hydroxyquinoline-sensitized anatase TiO2 powders to



Figure 19. Eosin Y-sensitized TiO2 for H2 evolution system in two-step water splitting. Reprinted with permission from ref 646. Copyright 2000 Elsevier.

generate hydrogen in a sacrificial water-reduction system containing EDTA as the electron donor using visible light.639 Gurunathan et al. investigated the photocatalytic activities for hydrogen production by Pt/SnO2 sensitized with various metal-free photosensitizers.619 These included acriflavin, Eosin Blue, rhodamine B, Rose Bengal, and fluorescein. Of all the photosensitizers used, Eosin Blue showed the maximum efficiency to sensitize SnO2 and evolved a greater amount of hydrogen, even higher than Ru(bpy)32+. Hirano et al. found that some porphine derivatives, such as tetrakis(4-carboxyphenyl)porphine (TPPC), tetrakis-(4-sulfonicphenyl)porphine (TPPS), and tetrakis-(4-pyridylphenyl)porphine (TPPPy) were all effective as photosensitizers.610 It was also found that TPPC/TiO2/Pt exhibited the highest activity for hydrogen evolution from water in the presence of EDTA as the electron donor. The principal reasons proposed for this enhanced activity include the degree of adsorption onto TiO2, the different electron densities in excited states, or redox potential. Chatterjee claimed that the efficacy of the photocatalytic system toward hydrogen evolution was quite possibly governed by the excited-state redox properties of the dyes adsorbed onto the surface of the TiO2 photocatalyst.640 A binaphthol complex was applied by Ikeda et al. to sensitize TiO2 for photocatalytic hydrogen evolution from TEA solutions under visible-light irradiation.641 The photonic efficiency of the photocatalytic reaction at 450 nm was estimated to be 0.02% for the binaphthol-modified TiO2 loaded with 0.1 wt % Pt. Abe et al. investigated the significant influence of solvent on hydrogen production over metal-free dye sensitized Pt/ TiO2 photocatalysts from a water-acetonitrile mixed solution containing an iodide electron donor under visible-light irradiation.613,642-644 The rates of H2 evolution decreased with increasing water content in the mixed solutions. This was due to the decreasing energy gap between the redox potential of I3-/I- and the HOMO level of the dye. However, when compared to merocyanine sensitized Pt/TiO2, a relatively high rate of H2 evolution was still observed over a coumarinsensitized Pt/TiO2 photocatalyst even in aqueous solution. This was because coumarin had a sufficiently positive HOMO level compared to the oxidation potential of I-. Shimidzu et al. reported extensive studies on visible-lightinduced photocatalytic water reduction using some xanthene dye-sensitized particulate Pt-loaded semiconductor catalysts.645 They found that heavy halogenated xanthene dyes, e.g., Rose Bengal, erythrosine, and eosine bluish, showed high quantum yields of hydrogen production for sensitized platinized semiconductors. However, they tended to photodehalogenate, whereas nonhalogenated xanthene dyes, e.g.,

uranine and rhodamine B, exhibited high durability against any photodeterioration but only moderate catalytic activities. Interestingly, it was also found that the addition of external halide ions improved the photocatalytic activities of nonhalogenated xanthene dye-sensitized platinized semiconductors. Abe et al. constructed a stable dye-sensitized photocatalyst system in water by a chemical fixation of xanthene dyes onto platinized TiO2 particles using a silane-coupling reagent.646 The Eosin Y-fixed Pt-TiO2 exhibited high efficiency and quite steady H2 production from aqueous TEA solution under visible-light irradiation for long periods. The quantum yield at 520 nm was determined to be ∼10%. Figure 19 shows the Eosin Y-sensitized TiO2 in a two-step water-splitting system for H2 evolution. Lu and co-workers systematically studied the Eosin Y-sensitized Ti-based photocatalysts for hydrogen generation from di- or triethanolamine aqueous solution under visiblelight irradiation (λ g 420 nm).647-653 Eosin Y-sensitized Rh/ TiO2,647 Pt/Na2Ti2O4(OH)2,649 and Pt/Ti-MCM-41652 showed relatively excellent photocatalytic activities and long-term stability for hydrogen production. Average quantum yields higher than 10% in the visible-light region were found. In particular, Eosin Y-sensitized Pt/Na2Ti2O4(OH)2, with a quantum yield up to 14.97%, showed good photocatalytic stability for hydrogen production over 100 h after 10 consecutive runs.649 Subsequently, a much higher quantum yield of 17.36% was obtained over Eosin Y-sensitized Ptloaded long titanic acid nanotubes. However, the destruction of the nanotube structure after long-time reaction led to a decrease in the hydrogen generation rate.653Additionally, the multilayer-Eosin Y-sensitized TiO2 via Fe3+ coupling was found to have a high light harvesting efficiency and photocatalytic activity for hydrogen evolution under visible-light irradiation. The maximum apparent quantum yield for hydrogen evolution is 19.1% from aqueous TEA solution.654 They also achieved efficient photocatalytic water reduction for hydrogen generation over Eosin Y-sensitized Pt/SiO2655 and Pt/MWCNT (multiwalled carbon nanotube)656 in the presence of TEA as the electron donor. Quantum yields up to 10.4% and 12.14%, respectively, were observed.

4.4. Developing Novel Single-Phase Visible-Light-Responsive Photocatalysts Even without using the modification technologies discussed above (ion doping, making solid solutions, and dye sensitization), many novel single-phase visible-light-responsive photocatalysts, mostly heterometallic oxides, have been fabricated successfully using metal-mediated band structure


Chen et al.

Figure 20. (A) UV-vis absorption spectra of In6NiTi6O22, In3CrTi2O10, and In12NiCr2Ti10O42 powder samples at room temperature. The dotted line shows the absorption spectrum of In12ZnGa2Ti10O42. (B) Schematic band structures of (a) In6NiTi6O22, (b) In3CrTi2O10, and (c) In12NiCr2Ti10O42. Reprinted with permission from ref 666. Copyright 2007 American Chemical Society.

engineering. In this section, we will focus on recent progress in the design of single-phase heterometallic oxides as novel visible-light-responsive photocatalysts. Of particular interest are materials with band structures mediated and band gap narrowed by d-, s-, and f-orbitals from the outer layer orbital configurations of d-block, p-block, and f-block metal ions, respectively.

4.4.1. d-block Metal Oxides The versatile features of the d orbitals of some transition metals for band gap narrowing have been demonstrated by doping such d-block transition metals into wide band gap photocatalysts to form a separate donor level in the forbidden band.353,354,525 The activities of the resulting doped photocatalysts are usually not high because the doping level can also serve as a recombination center for photogenerated electrons and holes. It is expected, therefore, that d-block transition metals could also contribute to the band gap narrowing of single-phase heterometallic oxide photocatalysts. In the study of Yin et al., the single-phase visible-lightdriven photocatalyst BaCrO4, with a band gap determined to be 2.63 eV, was synthesized by a solid-state reaction method.657 Since the Cr6+ 3d orbital was empty, the band structure of BaCrO4 was defined by the 3d level of Cr6+ and the O 2p level of the ligand O atom. As a result, the visiblelight transition was ascribed to the electronic excitation from the valence band composed of the O 2p orbitals to the conduction band composed of the Cr6+ 3d orbitals. Unlike the Cr 3d orbitals in BaCrO4, Cr3+ 3d orbitals in BaCr2O4 were partially filled and split into Cr 3d-t2 g and Cr 3d-eg orbitals. This split in band structure resulted in two cases of electron photoexcitations, namely, the photoexcitation from Cr 3d-t2 g to Cr 3d-eg and the photoexcitation from O 2p to Cr 3d-t2 g, evolving H2 and O2, respectively.658 Further reports of Cr-based oxides with different electronic structures of Cr 3d orbitals were conducted by Ouyang et al.659 In AgAlO2, the valence band and the conduction band were mainly constructed by Ag 4d and O 2p orbitals, and Ag 5s and 5p orbitals, respectively. The band gap was estimated to be 2.95 eV from the UV-vis spectra. When Al element in AgAlO2 was replaced by Cr, both AgCrO2 and Ag2CrO4 showed an obvious red shift of the absorption edge. The trivalent Cr ions in AgCrO2 owned three 3d-electrons, which were split to two groups, whereas the hexavalent Cr ions in Ag2CrO4 had no 3d-electrons. This was the reason AgCrO2 had double absorption bands and Ag2CrO4 only had a single absorption band in the visible-light region. Cr ions with different 3d orbitals had different effects on the band structure. Cr 3d orbitals in Ag2CrO4 only contributed to the conduction band,

whereas Cr 3d orbitals in AgCrO2 contributed to both valence and conduction bands. This was analogous to the previous reports on BaCrO4657 and BaCr2O4.658 Lv et al. developed a new photocatalyst, namely, LiCr(WO4)2, in which the Cr3d level contributed similarly to the formation of both the conduction and valence bands.660 It showed photocatalytic activity for H2 evolution under visiblelight irradiation. Ye et al. developed a new series of 3d transition metal Ni-containing photocatalysts, NiM2O6 (M ) Nb, Ta), which proved active for water splitting under visible-light irradiation.661 For NiM2O6, which contains two kinds of octahedra, NiO6 and MO6, the valence band energy was assumed to arise from both the O 2p orbitals of the NiO6 and MO6 octahedra. The valence band showed a value about 1.0 eV more positive than 2.94 (standard hydrogen electrode (SHE)) of O 2p levels. This resulted in the band gap narrowing of NiM2O6. It is believed that the Ni d-d transition between the Ni 3d-t2 g and Ni 3d-eg levels also played an important role in the visible-light photoexicitaion and photocatalytic activity of NiM2O6. Similar Ni d-d transitions were also observed in other Ni-containing heterometallic oxides such as BaNi1/3Nb(Ta)2/3O3,178,225 MLaSrNb2NiO9 (M ) Na, Cs, H),662,663 and Ca2NiWO6.664 In all these cases, such transitions appeared to be responsible for their visible-light absorption and visible-light-induced photocatalytic activities. Wang and co-workers systematically investigated the band structures of three oxide semiconductor photocatalysts, In6NiTi6O22, In3CrTi2O10, and In12NiCr2Ti10O42.665,666 They used different 3d transition metals with partially filled 3d orbitals to clarify the effects of the transition metal cations (Ni and/or Cr) on the photophysical and photocatalytic properties. As shown in Figure 20, the split Ni 3d orbitals in In6NiTi6O22 or the split Cr 3d orbitals in In3CrTi2O10 formed only a discrete band, whereas the coexistence of both Ni2+ and Cr3+ in In12NiCr2Ti10O42 enabled the formation of continuous conduction and valence bands through the hybridization of the split Ni 3d and Cr 3d orbitals with the Ti 3d/In 5s5p and O 2p orbitals. The formation of the continuous conduction and valence bands not only decreased the band gap energy but also increased the mobility of the photoinduced charge carriers. Thus, the photocatalytic activity of In12NiCr2Ti10O42 for hydrogen evolution under visiblelight irradiation was improved compared to those of In6NiTi6O22 and In3CrTi2O10. Silva et al. synthesized a series of Zn/Ti, Zn/Ce, and Zn/Cr layered double hydroxides (LDH) and tested them for the visible-light photocatalytic oxygen generation.667 Because of the chemical composition and in contrast to the (Zn/M)LDH (M ) Ti, Ce), the (Zn/Cr)LDH


containing Cr exhibited much greater light absorption in the visible region. The most active material was found to be the (Zn/Cr)LDH. Its apparent quantum yields for oxygen generation were 60.9% and 12.2% at 410 and 570 nm, respectively. Ye et al. found that the 3d transition metal V compound, InVO4, was effective for H2 evolution from pure water under visible-light irradiation.668 The InVO4 showed photocatalytic activity up to 600 nm, which is a much wider wavelength range than previously reported for In-based oxides such as InTaO4 and InNbO4. This was as expected from the conduction band composed of the less negative V 3d orbitals in InVO4, when compared to the Nb 4d orbitals in InNbO4 and the Ta 5d in InTaO4. It was reported that another vanadate, BiVO4, showed visible-light photocatalytic activity for O2 evolution from an aqueous solution containing either Ag+ or Fe3+ as electron acceptor.669-674 However, BiVO4 did not display photocatalytic activity for H2 evolution. This is because the conduction band composed of the V 3d orbitals was located at less negative potential than for H+ reduction to H2. Judging from the above results, it is possible that, depending on the chemical components and crystal structures of different vanadates, the V 3d level is either less negative or more negative than the H2 evolution potential. Some other V-containing oxide semiconductors, such as M2.5VMoO8 (M ) Mg, Zn),675 M3V2O8 (M ) Mg, Ni, Zn),676 CaBiVMO8 (M ) W and Mo),677 Bi2GaVO7,251 Bi2YVO8,252 and BiM2VO6 (M ) Cu and Zn),678,679 also displayed efficient visible-light absorption and photocatalytic activities. This is because the V 3d orbitals involved in the band structures act to lower down the conduction band, leading to band gap narrowing of these V-containing oxide photocatalysts. Yin et al. investigated a new series of visible-light-driven photocatalysts MCo1/3Nb2/3O3 (M ) Ca, Sr, and Ba) with an ABO3-type perovskite structure, in which the B site is occupied by Co2+ and Nb5+ randomly.680,681 In these compounds, the Co2+ 3d states, which were split into two main peaks, the lower t2 g state and the higher eg state, were strongly hybridized with the O 2p states to form the valence bands. As a result, the observed visible-light absorption for MCo1/3Nb2/3O3 was ascribed to the electronic excitations from the Co2+ t2 g state to the Nb5+ 4d state. Sun et al. reported that, in Bi5FeTi3O15, the Fe 3d band split into two main parts, corresponding to the Fe t2 g and the Fe eg, respectively.682 The photoexcitation from the hybridized O 2p + Fe t2 g + Bi 6s orbitals to the Fe eg orbitals were most probably responsible for the visible-light absorption of Bi5FeTi3O15. Because of the Fe 3d orbitals involved in the band structure, Ca2Fe2O5 was sensitive to visible light. Its band gap was estimated to be ∼1.86 eV from opitical absorption spectra. This could split pure water to generate H2 under visiblelight irradiation, after Ca2Fe2O5 was loaded with NiO.683 Kato et al. found that the band gaps of AgTaO3 and AgNbO3 were 0.6 eV smaller than those of NaTaO3 and NaNbO3, respectively, although their crystal structures of AgMO3 (M ) Ta, Nb) were similar to those of NaMO3.242 DFT calculations showed that a hybrid Ag 4d and O 2p orbital formed a valence band at a higher energy level than O 2p orbitals, and this resulted in the decrease in the band gaps of AgMO3 (M ) Ta, Nb). These findings made it possible to develop AgNbO3 as a good visible-light-driven photocatalyst with the ability to evolve H2 or O2 from water in the presence of sacrificial reagents. Similarly, the contribution of Ag+ to the valence band formation for R-AgVO3 led to a smaller band gap than in R-NaVO3, which was


responsible for the unnegligible photocatalytic activity for O2 evolution under visible-light irradiation.684 Keeping in mind the valence bands consisting of hybridized Ag 4d and O 2p orbitals, some noval Ag-based metal oxides, such as AgInW2O8,685 R-AgGaO2,686 Ag2ZnGeO4,687 and AgLi1/3M2/ 688 were developed as visible-light3O2 (M ) Ti and Sn), driven photocatalysts. The valence bands of these metal oxides are located at higher energy levels than those consisting of only O 2p orbitals. This is what leads to the narrowed band gaps and hence to the proposed visible-lightdriven photocatalytic activities.

4.4.2. p-block Metal Oxides In addition to the d-block transition metals, s-orbitals from the outer layer-orbital configurations of p-block metal ions are also effective to mediate the band structures. Tang and co-workers synthesized MIn2O4 (M ) Ca, Sr, Ba) semiconductors as potential visible-light-photoactive materials containing the InO6 octahedral structure.689,690 For these Incontaining oxides, the highest occupied band was composed of O 2p orbitals, which corresponded to the valence band. The lowest unoccupied band which was mainly composed of the In 5s orbitals, which corresponds to the conduction band. Taking this into consideration, the visible-light absorption was attributed to the photoexcition from the O 2p orbital to the In 5s orbital. However, for InMO4 (M ) Ta, Nb), which contains two kinds of octahedra, InO6 and MO6, the valence band was assumed to be a combination of both the O 2p levels of InO6 and NbO6 octahedrons. It showed ∼1.1 eV more positive than that of the O 2p levels.691-693 This is quite similar to the case in which the valence band of NiNb2O6 containing NiO6 and NbO6 octahedra was attributable to both the O 2p levels of NiO6 and NbO6 octahedra.661,694 The relatively positive valence band energy suggested that both InTaO4 and InNbO4 had suitable band structures and could respond to visible light. This was quite different from the visible-light photoexcition from O 2p orbital to In 5s orbital in MIn2O4 (M ) Ca, Sr, Ba). Zhou et al. prepared a visible-light-responsive polycrystalline Bi12TiO20 photocatalyst using a simple solid-state reaction between Bi2O3 and TiO2 powders.695 Its band gap was narrowed to be 2.78 eV through the introduction of the p-block transition metal Bi. The band structure of Bi12TiO20 originated from the Ti 3d band as well as the Bi 6s and O 2p hybridized band. This hybridization shifted the valence band upward, causing the band gap of Bi12TiO20 to be narrowed. Similarly, for some other Bi(III)-containing oxides, such as CaBi2O4,696,697 Bi2WO6,145,698,699 Bi2MoO6,700 BiSbO4,701 and Bi2MNbO7 (M ) Al, Ga, In),702,703 the proposed band structure of the valence bands also involved the hybridized orbitals between the Bi 6s and the O 2p orbitals. These played an important role in their visible-light absorption and photocatalytic activities. Kako et al. investigated the photophysical properties and band structure of NaBiO3 as a visible-light-driven oxide Bi (V) photocatalyst.704 They found that the band structure of the valence band in NaBiO3, mainly composed of the O 2p orbitals, was quite different from that of Bi(III)-containing oxides. The latter was composed of hybridized orbitals between the Bi 6s and the O 2p orbitals at the top of the valence band. This situation arose because the contribution of the empty Bi5+ 6s orbitals in NaBiO3 to the valence band was much smaller than the filled Bi3+ 6s orbitals in the Bi (III)-containing oxides.


Chen et al.

Figure 21. (A) Calculated total and partial density of states (DOS) of PbBi2Nb2O9. The conduction and valence bands of the compound consist of empty Nb 4d and occupied O 2p orbital, with the latter hybridized with Pb6s and/or Bi6s, giving the smaller band gap compared to compounds that do not contain Pb and Bi in their structure. (B) Schematic band energy diagram of lead- or bismuth-substituted perovskiterelated oxides. Reprinted with permission from ref 707. Copyright 2006 Elsevier.

Li and co-workers developed the two binary lead niobates, Pb3Nb2O8 and Pb3Nb4O13, as visible-light-sensitive photocatalysts.705,706 Compared to pure Nb2O5, the hybridization of the Pb 6s and O 2p orbitals in these lead niabates raised the position of the valence band edge and narrowed the band gap, leading to the observed visible-light responses. Kim and co-workers investigated the substitution effects of lead on the photophysical and photocatalytic properties of a range of UV-light-active photocatalysts: CaBi4Ti4O15, CaBi2Nb2O9, K0.5La0.5Ca1.5Nb3O10, and Sr3Ti2O7.707,708 They found that their lead-containing analogues (PbBi4Ti4O15, PbBi2Nb2O9, K0.5La0.5Ca0.75Pb0.75Nb3O10, K0.5La0.25Bi0.25Ca0.75Pb0.75Nb3O10, and PbTiO3) absorbed visible light and exhibited good photocatalytic activities for water decomposition under visible-light irradiation. This was attributed to the additional hybridization of the occupied Pb 6s and O 2p orbitals in such lead-containing compounds. This pushed up the position of the valence band, giving a smaller band gap compared to their respective lead-free counterparts as shown in Figure 21. Hosogi and co-workers found that SnNb2O6243,709 and SnNbO2,710 which contain Sn2+ with a 5s2 electron configuration, showed the photocatalytic activity under visible-light irradiation for H2 or O2 evolution from an aqueous solution containing methanol or AgNO3. The valence band level formed from a hybrid orbital of Sn 5s and O 2p was higher than that consisting of only O 2p orbitals. This made SnNb2O6 responsive to visible light. Furthermore, they developed a novel series of Sn2+-exchanged layered metal oxides, Sn2+/KTiNbO5, Sn2+/K4Nb6O17, Sn2+/CsTi2NbO7, Sn2+/K2Ti4O9, Sn2+/K2Ti2O5, and Sn2+/Cs2Ti6O13. These Sn2+-exchanged layered metal oxides had visible-light absorption bands and showed activities for H2 or O2 evolution from an aqueous solution containing a sacrificial reagent under visible-light irradiation.711 This was due to the

electronic transition from an electron donor level consisting of Sn 5s orbitals to conduction bands consisting of Ti 3d and Nb 4d orbitals. Of particular note is the contribution of the Sn 5s filled orbitals to the valence band structure of β-SnWO4, which causes a decrease in the band gap, leading to a novel visible-light active photocatalyst for H2 evolution from an aqueous methanol solution under visible-light irradiation.712

4.4.3. f-block Metal Oxides The introduction of rare earth 4f orbitals with a view to tuning the electronic structure has also been investigated for developing new visible-light-driven photocatalysts. Zou et al. investigated the effects of the rare earth elements on the band structures and photophysical properties of Bi2RNbO7 (R ) Y, rare earth).199,713 They found that the R 4f orbitals of the R3+ ions were very important for the band structures of these photocatalysts. The visible-light absorption was found to be based on the R 4f and Nb 4d band transition between the R3+ and Nb5+ ions. That is to say, the partly filled R 4f level in the rare earths could form a new energy level in the band structure, and the 4f-d transition resulted in the narrowed band gaps of these photocatalysts. Hwang et al. also found that the 4f band of rare earths greatly contributed to the band structures of R2Ti2O7 (R ) rare earth: La, Pr, Nd).127 The R 4f level in R2Ti2O7 was shifted to a lower energy as the number of 4f electrons increased. This decreased the band gap energy of both Pr2Ti2O7 and Nd2Ti2O7. A similar phenomenon was also discovered by Uno and co-workers for the R2M2O7 (R ) La, Pr, Nd, Sm, Gd, Dy, Ho, Er, and Yb; M ) Ti, Zr) photocatalysts.132,154 Because of the effect of the 4f orbital electrons, Sm2M2O7 (M ) Ti, Zr) and Nd2Zr2O7 were considered possible


candidates capable of responding to visible light for photocatalytic hydrogen production from water. Tian et al. developed a series of Ce-containing metal oxide photocatalysts K4Ce2M10O30 (M ) Ta, Nb), capable of evolving H2 and O2 from aqueous solutions, under visiblelight irradiation (λ > 420 nm), containing a sacrificial electron donor and acceptor, respectively.714 It was demonstrated that the conduction bands of K4Ce2M10O30 (M ) Ta, Nb) were mainly attributed to the Ta 5d (or Nb 4d) orbitals, while the valence bands were composed of hybridized O 2p + Ta 5d (or Nb 4d) and occupied Ce 4f orbitals. The latter made an essential contribution to the small band gap energy of these photocatalysts. The pyrochlore-type compound Sm2InMO7 (M ) Ta, Nb), with a 4f-d10-d0 configuration, was found to be a new stable visible-light-responsive photocatalyst for H2 evolution from water. The 4f-d10-d0 configuration was also proven useful for visible-light photocatalysis from the viewpoint of both the crystal and electronic structure.715,716

4.4.4. Miscellaneous Photocatalysts Recently, some phosphate semiconductors were reported to show good photocatalytic activity for water splitting under visible-light irradiation. For example, Ag3PO4 showed an extremely high quantum yield of ca. 80% at wavelengths less than ∼480 nm for O2 evolution from an aqueous silver nitrate solution.717 It was significantly higher than previously reported values.667 Li9Fe3(P2O7)3(PO4)2, prepared by a hydrothermal method, was proven to be active for photocatalytic H2 evolution under visible-light irradiation, where Iwas used as the electron donor.718 TiSi2, with a band gap range from 3.4 to 1.5 eV, was reported as a promising semiconducting catalyst for visiblelight-driven overall water splitting. The evolution of oxygen and hydrogen was facilitated with the formation of the catalytic centers on the surface of TiSi2 by photooxidation. Moreover, the reversible photoadsorption of oxygen onto the TiSi2 catalyst allowed the convenient separation of the hydrogen and oxygen products.719 A metal-free polymeric photocatalyst, carbon nitride (gC3N4), was developed by thermal condensation for efficient hydrogen or oxygen production from water under visiblelight irradiation with the assistance of a sacrificial reagent. By varying the thermal condensation conditions, the fine adjustment of the electronic and optical properties was possible. The band gap of the fully condensed graphitic carbon nitride was estimated to be 2.7 eV. Whereas the valence band was a combination of the HOMO levels of the melem monomer derived from the nitrogen pz orbitals, the conduction band was similarly connected to the LUMO of the melem monomer predominantly from the carbon pz orbitals.720 Homogeneous substitution of sulfur for lattice nitrogen within g-C3N4 gave rise to an increased valence bandwidth in combination with an elevated conduction band minimum and a slightly reduced absorbance. The resulting C3N4-xSx showed a H2 evolution rate 8.0 times higher than C3N4 under the irradiation of λ > 420 nm.721 The optical absorption of g-C3N4 was extended into the visible region up to about 750 nm after being copolymerized with barbituric acid.722 The modified g-C3N4 showed a remarkable improvement in H2 evolution activity compared to g-C3N4 under both UV and visible-light irradiation.722 A graphite oxide semiconductor photocatalyst was reported to steadily produce H2 under visible-light irradiation from an aqueous methanol solution, even in the absence of Pt as


the cocatalyst.723 The band gap energy of graphite oxide was dependant on the number of oxygenated sites and was estimated from optical absorption spectra to be 2.4-4.3 eV. The valence band edge of graphite oxide was mainly composed of the O 2p orbitals. The conduction band edge was mainly formed by the antibonding π*-orbitals and had a higher energy level than that needed for H2 generation.

5. Approaches for Efficient Photogenerated Charge Separation While visible-light-driven photocatalysts with proper band structures are currently developed using some modification technology or band engineering approaches as discussed above, the issue of photogenerated charge separation is another key factor strongly affecting the efficiency of the photocatalytic water-splitting process. Clearly, in order to increase the utilization rate of the photogenerated charges and obtain high photocatalytic water-splitting activities, the photogenerated charges must be efficiently separated to avoid bulk/surface charge recombination and transfer to the separated active sites on the surface of the photocatalysts. This is to ensure depression of the backward reaction of hydrogen and oxygen to form water. In this section, we will review the primary approaches and achievements to date for the efficient separation of photogenerated charges in the water-splitting process. We aim to present the numerous experimental and theoretical research results that have appeared over the past decades.

5.1. Cocatalyst Loading Transtition metals, especially the noble metals, are widely used as effective cocatalysts for photocatalytic water splitting. Taking Pt as an example, the processes of charge transfer between cocatalyst and host photocatalyst are described in Figure 22. When the noble metal is loaded onto the surface of the photocatalyst, the photogenerated electrons migrate to the surface of the host photocatalyst and are entrapped by the noble metal cocatalyst, because the Fermi energy level of noble metal is always lower than that of the semiconductor photocatalyst. Meanwhile, the photogenerated holes stay at the host photocatalyst and migrate to its surface. This results in the efficient separation of the photogenerated electrons and holes. Subsequently, the separately localized electrons and holes become involved in their roles as the reducer and oxidizer, respectively, in the photocatalytic reaction. Overall, the role played by the cocatalysts dispersed on the surface of the photocatalysts is extremely important. It improves the

Figure 22. Processes of charge transfer between host photocatalyst and cocatalyst, taking Pt as the example of cocatalyst.


Chen et al.

overall photocatalytic activity of the water splitting because it helps to promote charge separation, which in return reduces both bulk and surface electron/hole recombination. It also accelerates the surface chemical reaction by inhibiting the backward reaction.

5.1.1. Noble Metal Cocatalysts As one of the noble metals, Pt has been widely used as the cocatalyst in photocatalytic water splitting over many different kinds of semiconductors: oxides,71,80,92,186,724-726 (oxy)sulfides,489,490,727-730 and (oxy)nitrides.390,430,468,476,731 All have been shown to greatly enhance the photocatalytic activity for hydrogen evolution. Up until now, the highest photocatalytic activities for hydrogen production from water using visible-light irradiation are from photocatalysts loaded with Pt as the cocatalyst.732,733 Some other noble metals, such as Au,734-739 Ru,540,541,740-742 Pd,735,743-745 Ag,746-750 and Rh,751-754 have also been reported as efficient cocatalysts. Iwase et al. found that fine gold nanoparticles played an important role in the creation of active sites for H2 evolution and the enhancement of charge separation.167 In addition, the back-reaction between H2 and O2 to produce water on the Au cocatalyst was negligible in comparison to that on a Pt cocatalyst. This ultimately led to improved photocatalytic activities of some titanate, niobate, and tantalate photocatalysts for overall water splitting. Hara et al. reported the unusual enhancement of H2 evolution by Ru on a TaON photocatalyst under visible-light irradiation.740 It should be noted that, under identical conditions, other noble metals, such as Pt, Ir, and Rh, were ineffective in promoting any evolution of H2. The authors deduced that the electronic structure of the interface between the Ru particles and TaON possibly facilitated electron transfer from TaON to Ru. This ultimately gave an impetus to charge separation. Wu et al. investigated H2 production with low CO selectivity from the photocatalytic reforming of glucose in water on metal/TiO2 catalysts (metal ) Pt, Rh, Ru, Ir, Au, Ni, and Cu).755 The loaded metals, in particular Rh, were found to greatly enhance the rate of H2 production. This was attributed to the fact that the Schottky barrier formed at the metal and TiO2 interface could serve as an efficient electron trap, thus preventing photogenerated electron-hole recombination. The effect of the nature of the metal cocatalyst was interpreted in terms of different electronic interactions between the metal nanoparticles and the TiO2 surface.756 It was also reported that the smaller the Schottky barrier height at the metal/semiconductor junction, the greater was the electron flow from semiconductor to metal, thus leading to higher photocatalytic activity for hydrogen production.757 On the other hand, the synergistic enhancement effect of the Pt and Ru coloading on hydrogen evolution compared to that of either Pt or Ru alone was observed by Liu and co-workers.393,394 They considered that the superior activity of Pt/Ru-loaded LaTaON2 (or Y2Ta2O5N2) for H2 evolution was related to enhanced electron transfer from the conduction band of the photocatalyst to the Pt/Ru cocatalysts. This retards the possibility of electron-hole recombination in the valence band and improves the charge separation efficiency. When cocatalysts consisting of Au/Pd bimetallic nanoparticles with core/shell structures were loaded onto the TiO2 surface, selective H2 permeability by the Pd shell was believed to contribute to the selective donation of the photogenerated electrons to the protons. The result is greatly

Figure 23. Schematic illustration of the photoinduced events leading to water decomposition on Pt/RuO2-TiO2 composite catalyst. Reprinted with permission from ref 70. Copyright 1981 American Chemical Society.

enhanced photocatalytic production of H2 from aqueous ethanol solutions.758

5.1.2. Transition-Metal Oxide Cocatalysts Some transition-metal oxides such as RuO2187,244,257,277,577,759,760 and NiO109,110,175,206,761,762 are also well-known as efficient cocatalysts in water splitting. Domen and co-workers found that β-Ge3N4 alone exhibited little photocatalytic activity for water decomposition.24,277 However, when loaded with RuO2, the material became photocatalytically active under UV irradiation (λ > 200 nm). Maeda et al. found that the presence of RuO2 cocatalysts loaded on the g-C3N4 surface was indispensable not only for enhancing O2 evolution activity but also for suppressing the oxidative decomposition of the nitride catalyst.763 Similarly, IrO2 was also found to act as a water oxidation cocatalyst for water splitting.622,764,765 Borgarello and co-workers noted a pronounced synergistic effect in catalytic activity when both RuO2 and Pt are codeposited onto the TiO2 particles.308,606,766 Figure 23 depicts the photosplitting of water on Pt/RuO2-TiO2. It has been proposed that Pt is likely to yield an ohmic contact whereas a Schottky barrier may be formed by RuO2. This would direct the electron flow to the Pt sites while the holes would be trapped by RuO2,70 resulting in efficient charge separation and improved photocatalytic activity. Moreover, Teramura et al. found that the high dispersion of RuO2 nanoclusters on the catalyst surface was essential for improving the photoactivity for H2 and O2 evolution in overall water splitting.767 It was demonstrated that both Ru(IV) species and bulk RuO2 exhibited less activity for overall water splitting, whereas with RuO2 nanoclusters as cocatalyst, (Ga1-xZnx)(N1-xOx) displayed an improvement of H2 and O2 evolution. In a series of studies using (Ga1-xZnx)(N1-xOx), Maeda and co-workers loaded Cr-M (M being one of the transition metals, Fe, Co, Ni, Cu, Ru, Rh, Pd, Ag, Ir, or Pt) as a mixedoxide cocatalyst onto (Ga1-xZnx)(N1-xOx) using a coimpregnation method.768-771 The largest improvement in activity was obtained by loading the Rh-Cr mixed oxide (1 wt % Rh and 1.5 wt % Cr) with calcination at 623 K. It was proposed that loading the Cr-Rh mixed oxide facilitated the charge transfer from the host photocatalyst to the cocatalyst. It is also possible that, in addition, the loading promoted the creation of active sites for hydrogen evolution, which resulted in inhibited charge recombination and enhanced photocatalytic activity.772 Maeda and co-workers also developed noble metal/Cr2O3 core/shell nanoparticles as a cocatalyst for overall photocatalytic water splitting.773-775 Figure 24 shows


Figure 24. Schematic reaction mechanism of overall water splitting on Rh/Cr2O3-core/shell-loaded (Ga1-xZnx)(N1-xOx) and the corresponding processes on supported Rh nanoparticles and Cr2O3 nanoparticles. The impregnation of GaN:ZnO with Cr2O3 nanoparticles alone does not promote overall water splitting. H2 evolution occurs on Rh nanoparticles loaded on GaN:ZnO; however, in the presence of O2, this H2 reacts immediately with O2 on the Rh nanoparticles to form H2O. For Rh/Cr2O3-core/shell-loaded (Ga1-xZnx)(N1-xOx), H2 evolution occurs on the Cr2O3 shell, and O2 evolution occurs on the surface of GaN:ZnO bulk, thereby preventing water formation from H2 and O2 on Rh nanoparticles. Reprinted with permission from ref 773. Copyright 2006 WileyVCH.

a schematic reaction mechanism for overall water splitting on Rh/Cr2O3-core/shell-loaded (Ga1-xZnx)(N1-xOx). The mode of operation is quite different to cocatalysts such as the Rh-Cr mixed oxide, in which at least two roles are played simultaneously. In the Rh/Cr2O3 core/shell cocatalyst, the Rh core and the Cr2O3 shell worked independently. The Rh core promotes charge separation in (Ga1-xZnx)(N1-xOx) as well as tunneling electron transfer to the Cr2O3 shell, whereas the Cr2O3 shell provides catalytic active sites for H2 production, thereby preventing water formation from H2 and O2 on the Rh. The Rh core could be further replaced by other noble metals (Pd, Pt) as well as metal oxides (NiOx, RuO2, Rh2O3). This also resulted in enhanced photocatalytic activity for overall water splitting under visible-light irradiation.776 This enhancement in activity was primarily due to the suppression of undesirable reverse reactions (H2-O2 recombination and/or O2 photoreduction) and possibly the protection of the core component from chemical corrosion. This depended on the core type. Among the core materials examined, Rh species exhibited relatively high performance. Interestingly, with assistance of Mn3O4 nanoparticles coloading, the photocatalytic activity for overall water splitting was improved for (Ga1-xZnx)(N1-xOx), which was modified with core/shell-structured Rh/Cr2O3 nanoparticles. The Mn3O4 nanoparticles functioned as O2 evolution sites, and Rh/Cr2O3 nanoparticles hosted H2 evolution sites.777 When NiO acts as the cocatalyst for photocatalytic water splitting, an activation pretreatment is generally necessary for NiO-loaded photocatalysts in order to obtain high activities.175,353,778 A reduction-reoxidation treatment produces a double-layered NiO/Ni structure on the surface of the photocatalyst. Because NiO has a lower Fermi level in comparison to metallic Ni, this double-layered structure facilitates the electron transfer from the photocatalyst material to the Ni layer and then onto the NiO layer of the H2


evolution sites. The result is the efficient charge separation for water splitting and the suppression of the backward reaction of water splitting on the metallic Ni surface. Tian et al. investigated the effects of nanosized Pt, RuO2, and NiOx loading onto the visible-light-driven photocatalysts K4Ce2M10O30 (M ) Ta, Nb) for hydrogen evolution from water.779 The photocatalytic activities of evolving H2 were markedly promoted by cocatalysts loading, in particular, the NiOx loading with the formation of the NiO/Ni doublelayered structure. This was attributable to enhanced electron migration from the conduction band of the photocatalyst to the NiO/Ni cocatalyst. Hwang et al. prepared a series of metal oxide (MOx, M ) Ni, Pt, Cs, Bi, Fe, Pb, Ce)-loaded Sr2Nb2O7 photocatalysts using the impregnation method and following reduction-oxidation treatment.780 Of these metal oxides, the NiOx cocatalyst showed the highest activity for water splitting. The reduction-oxidation pretreatment for the formation of a double-layered structure was important to achieve the high activity especially for NiOx-loaded catalysts. This could be ascribed to the more efficient electron-hole separation as a result of the role of nickel played in the p-type/n-type junction between NiOx and Sr2Nb2O7 as formed in the reduction-oxidation pretreatment. However, this marked dependence of photocatalytic activity on pretreatment conditions was not observed for any other metal oxides in this study. To improve the photocatalytic activity of H2O decomposition, various kinds of metal oxides (MOx: M ) Cr, Mn, Fe, Co, Cu, Ru, Ag, Ce, Sm, and Pb) were introduced into the NiOy-K2La2Ti3O10 catalyst as a second component of the cocatalyst together with NiOy. Only the CrOx-NiOy-K2La2Ti3O10 catalyst showed higher photocatalytic activity and durability for longer periods of irradiation than the parent NiOy-K2La2Ti3O10.781

5.1.3. Nonmetal-Oxide Cocatalysts In addition to the noble metals and the transition-metal oxides, some other compounds, such as the transition-metal sulfides, have also been developed as novel cocatalysts. Zong and co-workers developed MoS2 as a novel cocatalyst for photocatalytic hydrogen evolution.782,783 They found that the CdS activity was enormously increased by loading with MoS2, even higher than that of Pt-loaded CdS under the same reaction conditions. The better coupling between the structures and electronic configurations of MoS2 and CdS together, and the formation of junctions between CdS and MoS2, improved the charge separation and were mainly responsible for the high activity of this MoS2/CdS catalyst. MoS2 nanoparticles cocatalysts were also found to be effective in H2 evolution over CdSe nanoribbons.784 The MoS2 activated the photocatalyst by reducing the electrochemical proton reduction overpotential.784 Li and co-workers found that the photocatalytic activity of CdS could be enhanced significantly by loading a small amount of a noble metal sulfide (PdS, Rh2S3, Ru2S3), as well as a noble metal (Pt, Pd, Ru, Rh).733,785 Moreover, codeposition of Pt with other noble metal sulfides on CdS demonstrated further enhanced photoactivity in hydrogen production; the photocatalytic activity of CdS codeposited with Pt and PdS was greater than those of Pt/ CdS and PdS/CdS. This synergistic effect between the Pt and PdS cocatalysts could be explained by the fact that the two cocatalysts may facilitate separation of the photogenerated electrons and holes on the photocatalyst. Tabata et al. found that dispersion of transition metal sulfides such as NiS, FeS, Ru2S3, Ag2S, CoS, and PdS, into


Chen et al.

the CuGa3S5 photocatalyst solution also increased the photocatalytic activity.498 The transition metal sulfides were believed to accept electrons from the excited state of CuGa3S5 and reduce H+ into H2 when transition metal sulfides and CuGa3S5 particles collided with each other. Jang et al. proved that tungsten carbide (WC) had potential as an alternative cocatalyst for photocatalytic hydrogen production.786 Under visible-light irradiation, the WC/CdS photocatalyst showed excellent photocatalytic activity for hydrogen production from water, comparable to that of conventional Pt/CdS. This was because WC provided active sites for hydrogen evolution and promoted fast migration of the photogenerated electrons from CdS to WC. This resulted in efficient charge separation and enhanced photocatalytic activity.

5.2. Semiconductor Combinations The semiconductor combination approach has been shown to be another effective method for improving photocatalytic activity through better photogenerated charge separation with a formation of a heterojunction structure. As is well-known, CdS, which is a fascinating visiblelight-driven photocatalyst for hydrogen production, is very unstable toward photocorrosion, as a result of serious selfoxidation by the photogenerated holes in the valence band. To improve its photocatalytic activity and stability, CdS has been embedded in different kinds of inert matrices,787-793 as well as combined with other semiconductors of different band energies, such as TiO2,794,614 ZnO,614,796-798 LaMnO3,799 and KNbO4.800,801 Among these composites, CdS-based semiconductor combination systems, CdS/TiO2 has attracted the most extensive research.802-810 Charge separation in a CdS/ TiO2 system, as shown in Figure 25,811,812 has been investigated in several detailed studies.614,811-814 Both the conduction and valence band edges of CdS are at more negative potentials than those of TiO2. Under visible-light irradiation, the photogenerated electrons in the CdS particles quickly transfer to TiO2 particles, whereas photogenerated holes stay in CdS. This facilitates the electron-hole separation and prevents the charge recombination, improving the photocatalytic activity. Tada et al. developed an anisotropic CdS-Au-TiO2 heterojunction, in which CdS, TiO2, and the electron-transfer medium (Au) were all spatially fixed.815 This threecomponent system exhibited a high photocatalytic activity, far exceeding those of the single- and two-component systems. This is a result of vectorial electron transfer driven by the two-step excitation of TiO2 and CdS. Park et al. investigated the effects on visible-light-driven hydrogen production of varied combinations of CdS, TiO2, and Pt in hybrid photocatalysts (Figure 26).816 They found that direct particle-to-particle contact of CdS and TiO2, and photodepo-

Figure 25. Charge separation in CdS/TiO2 semiconductor combination system under visible-light irradiation. Reprinted with permission from ref 812. Copyright 2009 Wiley-VCH.

Figure 26. Illustrative diagrams of the electron transfers in the hybrid photocatalysts. (a) Pt-CdS; (b) CdS + Pt-TiO2 (physically mixed); (c) CdS/(Pt-TiO2); (d) Pt-(CdS/TiO2); (e) TiO2/(Pt-CdS); (f) CdS/TiO2 + Pt. Reprinted with permission from ref 816. Copyright 2008 The Royal Society of Chemistry.

sition of Pt on the TiO2 particle surface, which resulted in the vectorial electron transfer of CdS f TiO2 f Pt (Figure 26c), was necessary to achieve efficient charge separation and transfer and hence observed the highest photoactivity of the CdS/(Pt-TiO2) hybrid catalyst. Because of the fact that the semiconductor combination has been proven to play a beneficial role in the improvement of photogenerated charge separation, many other different kinds of semiconductor combination systems have been developed for photocatalytic hydrogen production from water. Wang et al. developed a novel Zn-doped Lu2O3/Ga2O3 composite photocatalyst for stoichiometric water splitting.255 It was proved to have great advantage over the individual precursor materials owing to its enhanced charge-separation ability. Similarly, the TiO2/SnO2 mixed oxide showed enhanced photocatalytic activity for hydrogen generation compared to pure TiO2.83 Guo and co-workers found that the TiO2-xNx-WO3 composite photocatalyst showed higher hydrogen production activity under visible-light irradiation than either TiO2-xNx or WO3 alone.817,818 Again this was attributed to the efficient charge separation of photogenerated electrons and holes. Zou and co-workers reported a novel Cr-doped Ba2In2O5/ In2O3 system, which was properly bridged by an ohmic contact.819 It turned out to be a novel composite photocatalyst with enhanced activity for water splitting when compared to the individual components. The photoinduced charge carrier separation and migration were promoted by the potential offsets between the band edges of individual materials Cr-Ba2In2O5 and Cr-In2O3. On the basis of a similar electron transfer mechanism, In2O3/NaNbO3 was also found to be advantageous for both photocatalytic H2 evolution under visible-light irradiation and pure water splitting under UV irradiation.820 Ou et al. successfully synthesized a visible-light-driven MWNT-TiO2 composite catalyst using MWNTs dispersively grown on the surface of TiO2.821 In this system, efficient charge separation and effective photocatalytic H2 evolution resulted when the photogenerated electrons of the MWNTs transferred quickly to the conduction band of the TiO2 under visible-light irradiation. Similarly, in a Bi2S3/TiO2 system, the enhanced photoactivity was


Figure 27. Relative quantum efficiency for hydrogen production, obtained from platinum-tipped unseeded CdS rods (yellow), and five different samples of platinum-tipped seeded rods, with seed diameters of 3.1 (red) or 2.3 nm (green). Underneath each bar is the corresponding average sample length. Reprinted with permission from ref 824. Copyright 2010 American Chemical Society.

ascribed to photoelectron transfer from the conduction band of Bi2S3 to the conduction band of TiO2, resulting in water reduction.822 Silva et al. developed a novel Pt-interlinked hybrid composite of cubic-phase CdS (c-CdS) and hexagonal-phase CdS (hex-CdS).823 In order to explain the relative order of photocatalytic activity found, c-CdS/Pt/hex-CdS > Pt/c-CdS/ hex-CdS > Pt/hex-CdS > hex-CdS > c-CdS/hex-CdS > c-CdS, they concluded that the formation of a potential gradient at the interface between the cubic and hexagonal CdS, and the interlinkage of quantum-sized cubic CdS and bulk-phase hexagonal CdS with Pt, were necessary to achieve the efficient charge separation and transfer. This was quite similar to the CdS/Pt/TiO2 semiconductor combination system investigated in their previous study.816 Recently, Amirav and Alivisatos designed a multicomponent nanoheterostructure for efficient photocatalytic hydrogen production composed of a Pt-tipped CdS rod with an embedded CdSe seed.824 In such structures, holes were threedimensionally confined to the CdSe seed, whereas the delocalized electrons were transferred to the metal tip. Consequently, the electrons were separated from the holes over three different components and by the tunable physical length of the CdS rod. By tuning the nanorod heterostructure length and the seed size, as shown in Figure 27, the hydrogen production activity was significantly increased compared to that of the unseeded rods. This structure was found to be highly active for hydrogen production, with an apparent quantum yield of 20% at 450 nm. There was also a demonstrated improved stability compared to CdS rods without CdSe seeding. The incorporation of a guest semiconductor into the interlayers of a lamellar compound for fabricating an intercalated composite semiconductor has been considered as a promising method for the enhancement of the photocatalytic activity. The idea is that in this guest-host semiconductor combination system, the recombination between the photoinduced charge carriers is effectively suppressed due to the quick charge transfer from the guest to the host semiconductor.825-829 In the past few years, some transition metal oxides with semiconducting host layers have been shown to be generally promising candidates for use as intercalation hosts in photocatalysts.830-834 Wu and coworkers reported the intercalation of nanosized oxides (i.e.,


Figure 28. Mechanism of photocatalytic H2 evolution on CdSintercalated layered composites loaded with Pt. Photogenerated electrons in CdS quickly transferred to host layers through the nanostructure, and the recombination between the photoinduced electrons and holes was effectively suppressed. Reprinted with permission from ref 842. Copyright 2007 IOP Publishing Ltd.

Fe2O3 or TiO2) into the interlayer of various layered metal oxides (i.e., H4Nb6O17, HNb(Ta)WO6, or HLaNb2O7).835-838 When compared to the unintercalated materials, these intercalated composite semiconductors possessed higher photocatalytic activities for hydrogen production in the presence of methanol as a sacrificial agent under UV or even visible-light irradiation. This was ascribed to an effective separation of the photogenerated electrons and holes by electron transfer from guest semiconductor to the host layer. Subsequently, Jang et al. intercalated nanosized Fe2O3 particles into the interlayers of HTiNbO5 and HTiTaO5 using successive intercalation reactions.839 They found that the strong electronic interaction between the guest nanoparticles and the host layers, which was derived from the high electron deficiency of the nanosized Fe2O3 particles, could work favorably for photocatalysis because of an efficient electronhole separation. However, in contrast to the results of Wu et al.,838 this Fe2O3-intercalated layered composite semiconductor did not lead to photocatalytic H2 production from water reduction but instead to a high activity for oxygen production from water oxidation under visible-light irradiation. To improve their photocatalytic stability and photoactivity, sulfides, such as CdS, have also been intercalcated into the interlayers of some layered metal oxides. Shangguan et al. prepared a series of CdS-intercalated metal oxides using direct Cd2+ exchange followed by a sulfurization process.840-842 They found that the photocatalytic activities for hydrogen evolution of such CdS-intercalated composites were superior to those of CdS alone or to a physical mixture of CdS and the metal oxides. This activation effect was attributed to the quick transfer of the photogenerated electrons from CdS to the metal oxides through the layered nanostructure, as shown in Figure 28. The photogenerated charge recombination was effectively suppressed. Sato and co-workers investigated the photocatalytic activities of intercalated materials based on layered metal oxides (i.e., Ca2-xLaxNb3O10, HNbWO6, or HLaNb2O7) as the host and Cd0.8Zn0.2S as the guest.843-845 Fabrication involved successive intercalation and exchange reactions. Under visible-light irradiation, the hydrogen production activities of these Cd0.8Zn0.2S-intercalated composite photocatalysts were superior to those of unsupported Cd0.8Zn0.2S. They were further enhanced by the coincorporation of Pt. Clearly efficient charge separation resulted from the heterogeneous electron transfer from guest Cd0.8Zn0.2S


to host oxide layers, and this played an important role in the enhancement of the photocatalytic activity for hydrogen evolution. It has also been noted that the encapsulation of guest semiconductors into the micro/mesostructured semiconducting host materials is effective for photogenerated charge separation and thus leads to the improved photocatalytic activity of such semiconductor combination systems. Using ion-exchange and sulfurization processes, Guan and coworkers successfully incorporated CdS nanoparticles into the microchannels of ETS-4 and ETS-10, which have the photocatalytically active -Ti-O-Ti- quantum wires in their frameworks.846,847 The resulting CdS/ETS composite system showed better photocatalytic activity and stability than CdS nanoparticles for hydrogen production under visiblelight irradiation. This was interpreted in terms of more efficient charge separation due to the transfer of the photogenerated electrons from the CdS nanopaticles to the -Ti-O-Ti-O- nanowires. Similarly, Shen and Guo encapsulated CdS and In2S3 nanoparticles into the mesopores of Ti-MCM-41.848,849 Under visible-light irradiation, the composite materials exhibited greater and more stable photocatalytic activity for hydrogen evolution than either bulk CdS or In2S3. Jing and Guo reported the deposition of quantum-sized WS2 onto the channel surface of crystalline mesoporous TiO2.850 It was postulated that under visible light only electrons transferred from nanosized WS2 to the TiO2 host. This resulted in the effective charge separation of electrons and holes photogenerated in the WS2, and thus the efficient photocatalytic activity for hydrogen production on the WS2/TiO2 semiconductor combination system. Shortly afterward, they developed a novel composite CdS/meoporous zirconium titanium phosphate (ZTP) photocatalyst for working under visible light by a two-step thermal sulfidation procedure. In this system, the conduction band of ZTP could be continuously adjusted by choosing different Zr/Ti ratios. Therefore, by adjusting the conduction band of the photoactive ZTP to achieve an optimal optical match between the CdS guest and the ZTP host, highly efficient charge separation and hydrogen production were achieved over the designed CdS/ZTP composite photocatalyst. The highest quantum yield for this composite photocatalyst (with a Zr/ Ti ratio of 1:3 in the ZTP host) at 420 nm as measured in experiments reached 27.2%.851 Narrow band gap semiconductors, such as CdS852-854 and Cr2O3,855 have also been incorporated into the nanotubular semiconducting host, generally titanate nanotubes (TiO2NTs), to develop high-efficiency composite photocatalysts for hydrogen production. Among them, the CdS/TiO2NTs composite photocatalyst, in which homogeneously distributed CdS was incorporated inside the TiO2NTs, showed a high photoactivity for hydrogen production from water containing sulfide and sulfite ions as hole scavengers under visible-light irradiation, with the apparent quantum yield of ∼43.4% at ∼420 nm. The potential gradient at the interface between the CdS nanoparticles and TiO2NTs helped to facilitate the photoelectron diffusion from CdS particles toward the TiO2NTs and led to high photocatalytic activity of hydrogen production.854 It has been demonstrated that, in both photovoltaic and photoelectrochemical (PEC) cells, improved performance and higher conversion efficiency can be obtained by using diode structures. These were combined from suitable n-type photoanodes and p-type photocathodes856-858 and led to

Chen et al.

Figure 29. Reaction scheme of the photoinduced water splitting over the coupled p-type Cu2O and n-type WO3 photocatalysts in a suspension system. Reprinted with permission from ref 867. Copyright 2008 Elsevier.

efficient electron-hole separation with the suppression of energy-wasteful charge recombination.859-866 A p-Cu2O/nWO3 coupling system was developed by Hu et al. with a view to avoiding back-reactions of the photoinduced charges.867 It resulted in higher photocatalytic hydrogen production. The reaction scheme of photoinduced water splitting over coupled p-type Cu2O and n-type WO3 photocatalysts in a suspension system is shown in Figure 29. Trari and co-workers synthesized a series of p-n heterojunction for use under visible-light irradiation, such as p-CuMO2/n-Cu2O (M ) Mn, Cr),868,869 p-CuAlO2/n-TiO2,870 p-CuFeO2/n-SnO2,871 and p-ZnFe2O4/n-SrTiO3,872 for photocatalytic hydrogen production from aqueous solutions containing hole scavengers. In these p-n semiconductor systems, photogenerated electrons and holes separated efficiently and were involved in photocatalytic reduction and oxidation, respectively. Jang and co-workers successfully fabricated p/n-typed photocatalytic diodes, n-CdS/p-AgGaS2,873 p-AgGaS2/n-TiO2,874 and p-CaFe2O4/n-MgFe2O4.875 All of these p/n photocatalysts exhibited higher visible-light activities for hydrogen production than the single p- or ncomponent. This was mainly due to efficient charge separation, which was caused by the rectification of photogenerated electrons and holes. Kim et al. reported that photocatalytic nanodiodes formed from p-CaFe2O4/n-PbBi2Nb0.9W0.1O9 yielded greatly enhanced and stable photocatalytic activity for water oxidation under visible light compared to the single-component photocatalyst.876 In this p-n photocatalytic nanodiode, enhanced and stable photocatalytic activity was achieved because, under the influence of the internal electric field, the photogenerated holes moved to the p-CaFe2O4 side and the electrons moved to the n-PbBi2Nb1.9W0.1O9 side, leading to more efficient charge-carriers separation. In a later study, the authors adopted the concept of a p-type/n-type diode structure with an Ohmic junction and fabricated the psemiconductor/metal/n-semiconductor structured composite photocatalyst n-WO3/W/p-PbBi2Nb1.9Ti0.1O9 for more efficient utilization of visible-light photons.877 This nanocomposite photocatalyst showed unprecedented high activity for the photocatalytic oxidation of water under visible-light irradiation, with quantum yield estimated to be ca. 41%. Figure 30 shows the working principle of WO3/W/ PbBi2Nb1.9Ti0.1O9 nanocomposite photocatalyst. It had efficient electron-hole separation and higher net photon energies available for redox reactions through creation of the metal W layer needed to separate the p-type and n-type



Figure 31. Junction structure formed between the anatase and rutile phase. Reprinted with permission from ref 73. Copyright 2008 Wiley-VCH.

Figure 30. Working principle of n-WO3/W/p-PbBi2Nb1.9Ti0.1O9 nanocomposite photocatalyst. Reprinted with permission from ref 877. Copyright 2006 American Institute of Physics.

semiconductors to yield an Ohmic contact in between. This led to more efficient photocatalytic activity than the p-type/ n-type junction structure lacking this Ohmic layer.877

5.3. Modification of Crystal Structure and Morphology In general, charge separation and transfer of photogenerated electrons and holes are strongly affected by the crystal structural features of the materials, namely, crystallinity, defects, and any crystal structure distortion. Additionally, surface properties such as particle size, surface area, surface structure, and active reaction sites, which are mainly related to the morphology of the materials, are also important. Thus, a respectable research effort has been dedicated to both the modification of crystal structure and morphology of the photocatalysts with the view to improve more efficient charge separation. This has had great success in the enhancement of photocatalytic activity for water splitting.

5.3.1. Modification of Crystal Structure It has been well demonstrated that the crystal structure of TiO2 plays a significant role in photocatalysis.795,878-882 In photocatalysis, for pure-phase TiO2, the anatase phase was considered to be more active than the rutile phase.795,878 In anatase TiO2, the photoexcited electrons could be trapped in oxygen vacancies of the anatase structure.72 This made them easier to transfer to an electron trap, such as Pt particles on the surface, to participate in the photocatalytic reaction, preventing electron-hole recombination in photocatalysis. On the other hand, the poor photoactivity of rutile TiO2 was due to the fact the electrons are trapped within intrinsic defects of the rutile structure where they were deexcited by near-infrared emission.72 Meanwhile, enhanced activity was observed on mixed-phase TiO2 photocatalysts relative to the corresponding pure phases.73,883-887 Taking an anatase/rutile mixed-phase TiO2 as an example, Figure 31 reveals a junction structure formed between the anatase and rutile phases. The migration of electrons across a phase junction (as shown in Figure 32) was beneficial for charge separation, thereby enhancing the photocatalytic activity for hydrogen evolution.73,888 Furthermore, the high crystallinity of anatase TiO2, which had fewer lattice defects, was reported to have a positive effect on the photocatalytic activity for H2 production. Good crystallinity led to significant enhancement

Figure 32. Proposed pathway of electrons during photocatalytic H2 evolution over a mixture of anatase and rutile TiO2 nanoparticles. The amount of electron transfer proceeds predominantly in the order of solid thick arrow > thin solid arrow > unfilled arrow. Note: For simplicity, the formation of hydroxymethyl radicals ( · CH2OH) by hydroxyl radicals ( · OH) is represented by the hole oxidation step. Reprinted with permission from ref 888. Copyright 2010 American Chemical Society.

of the electron transport properties, whereas lattice defects behaved as recombination centers for the photoinduced electron/hole pairs with a concomitant decrease in the photocatalytic activity.889,890 Fu et al. studied the In2S3 samples with different crystal structures.891 Their results showed that the indium vacancyordered tetragonal In2S3 was inactive for hydrogen generation, whereas the vacancy-disordered cubic In2S3 exhibited stable photoactivity under visible light.891 Amano et al. reported that, owing to the suppression of the fast recombination of electron-hole pairs, the photocatalytic activity of visible-light-responsive Bi2WO6 was greatly enhanced by crystallizaiton under a hydrothermal treatment, when compared to the negligible photocatalytic activity of amorphous Bi2WO6.892 Noda et al. demonstrated that the high photocatalytic activity of crystallized mesoporous Ta2O5, for overall water splitting, was attributable to the efficient transfer of the excited electrons and holes from inside the catalyst to the surface through the thin-walled crystalline phase.893 Domen and co-workers found that high-pressure treatment of β-Ge3N4 and Ta3N5 under ammonia was effective for reducing the defect sites and/or structural imperfections both in the bulk and on the surface, resulting in enhanced photocatalytic activities for water splitting.278,279,894 Postcalcination at moderate temperatures was found to be effective for improving the activities of (Ga1-xZnx)(N1-xOx) and (Zn1+xGe)(N2Ox) as visible-light-driven photocatalysts for overall water splitting. This was also attributed to a reduction in the density of lattice defects in the catalyst materials, which in return reduced the number of sites available for the


recombination of the photogenerated electrons and holes.575,579 A H2S post-treatment was applied by Jang and co-workers for the synthesis of pure sulfide-type photocatalysts, with high crystallinities. Because of the suppressed charge recombination, the obtained AgGaS2 exhibited high photocatalytic activity for hydrogen production under visible light.496 Good crystallinity and fewer crystal defects were also discovered to benefit bulk electron-hole separation as well as the efficient photocatalytic activity of CdS.895 Li et al. found that suitable photoetching could notably increase photocatalytic activity of Pt/CdS for hydrogen evolution by removing selectively grain boundary defects that were the recombination centers for photoinduced electron-hole pairs.896 Maeda et al. found that Ta3N5 nanoparticles with a lower density of defect sites exhibited enhanced photocatalytic activity for H2 evolution.472 They also reported the positive effect of a monoclinic-ZrO2 modification on the photocatalytic H2 evolution activity of TaON under visiblelight irradiation. Both prior incorporation of a zirconium species into ZrxTa1-xO1+xN1-x solid solutions and surface modification of TaON with monoclinic-ZrO2 suppressed the formation of surface defects by inhibiting tantalum reduction during nitridation even though the ZrO2 component itself did not undergo nitridation.897,898 The photocatalytic performance of semiconducting nanocrystals is also highly dictated by their crystal planes. For TiO2, different groups have reported the tailored synthesis of anatase single crystals with a high percentage of the highly reactive {001} facets. These showed superior photoreactivity compared to P25 as a benchmarking material.899-905 Wu et al.905 and Li and Xu906 reported that nanostructured anatase TiO2 with a large percentage of other exposed high-energy facets, {010} and {100}, respectively, exhibited much higher activities than that of commercial anatase powders. Pt/TiO2 nanosheets with exposed (001) facets fabricated by a hydrothermal treatment of tetrabutyl titanate and hydrofluoric acid mixture were shown to exhibit a much higher photocatalytic activity for H2 evolution than Degussa P-25 TiO2 and pure TiO2 nanoparticles because of the synergistic effect of surface fluorination and exposed (001) facets.907 Zhao et al. prepared WO3 octahedra with {111} surface facets, which were covered and stabilized with a thin tungstic acid layer.908 The as-prepared octahedra exhibited high visible-light-driven photocatalytic activity for oxidation of H2O to O2. This was due to the high adsorption capacity of the tungstic acid sheath for Ag+ as the electron acceptor and the efficient water oxidation at the high-energy {111} facets. Nian et al. succeeded in controlling the crystalline texture of Cu2O by varying the electrodeposition conditions.909 The Cu2O grown with a [111] out-of-plane texture had a better photocatalytic performance in water splitting for hydrogen production than that with a [110] texture, due to the large exposure area of {111} facets of Cu2O crystalline.910,911 As shown in Figure 33, Xi and Ye deemed that the exposed {001} facets of the monoclinic BiVO4 nanoplates led to a remarkable enhancement of the visible-light photocatalytic oxidation of water for O2 generation.912 Yin et al. found evidence for the possible role of lattice vibrations in the photocatalytic H2 production activity of BaM1/3N2/3O3 (M ) Ni, Zn; N ) Nb, Ta).178 They found that the lower photocatalytic activity resulted from the deviation of the bond angle M-O-N from 180°. This change increased the migration energy of the charge carriers,

Chen et al.

Figure 33. (a, b) Low- and high-magnification field emission scanning electron microscopy (FESEM) image of the m-BiVO4 nanoplates. (c) Low-magnification transmission electron microscopy (TEM) image of the m-BiVO4 nanoplates. (d) High-resolution TEM (HRTEM) image of the m-BiVO4 nanoplate. (e) Photocatalytic O2 evolution from an aqueous AgNO3 solution (0.05 M, 270 mL) under visible-light irradiation (λ > 420 nm) over various photocatalysts (0.1 g). Reprinted with permission from ref 912. Copyright 2010 The Royal Society of Chemistry.

thus hindering their migration of the charge carriers and leading to a higher possibility of recombination between the photogenerated electrons and holes. Similarly, in the study of Kudo et al.,21 Sr2Ta2O7 displayed a higher photocatalytic activity for water splitting than Sr2Nb2O7. As the bond angle of O-Ta-O in Sr2Ta2O7 was closer to 180° than that of O-Nb-O in Sr2Nb2O7, the charge carriers in Sr2Ta2O7 moved more easily than those in Sr2Nb2O7. On the other hand, Sr2Nb2O7 was also active for the water splitting even if it was a niobate. This was due to a dipole moment along the perovskite layers resulting from the distortion of NbO6 octahedra, which, it was suggested, could enhance the charge separation of the photogenerated electrons and holes in Sr2Nb2O7. In fact, a dipole moment of this type, due to the distortion of TiO6 octahedra in some titanates such as BaTi4O9, was reported previously by Inoue and co-workers as being important for the charge separation in photocatalytic water splitting.101,913,914 In their later studies,258-260,263,265 the prominent effect of crystal structure distortion on photocatalytic activity was also reported for other metal oxide photocatalysts: Zn2GeO4, MIn2O4 (M ) Ca, Sr), M2Sb2O7 (M ) Ca, Sr), and AInO2 (A ) Li, Na). It was demonstrated that the metal oxides consisting of distorted structural units with dipole moments were all photocatalytically active in water decomposition, whereas distortion-free oxides exhibited negligible activity. Structure distortion was clearly effective for charge separation. Figure 34 compares the correlation between photocatalytic activity and dipole moment. Recently, Shen et al. found that, in hydrogen evolution, the photocatalytic activity for ZnIn2S4 was greatly affected by the crystal plane space along the c-axis; the increasing d (001) space greatly improved its photocatalytic activity of ZnIn2S4.377,915 They concluded that the structural distortion of ZnIn2S4 induced a dipole moment through increasing the d (001) space. Since the internal fields caused by the dipole moment were considered to be useful for the charge separation of the photogenerated electrons and holes, this in turn proved effective in promoting the photocatalytic activity.

5.3.2. Modification of Size and Morphology It is well-known that particle size is a crucial factor in the dynamics of electron/hole recombination (including bulk recombination and surface recombination) processes, especially in semiconductor nanomaterials, and that the move-


Figure 34. Dipole moments in (a) SrIn2O4 and (b) BaTi4O9, and (c) correlation between photocatalytic activity and dipole moment. The octahedral structures represent InO6 units. The indates with dipole moments are photocatalytically active, whereas the distortionfree indates exhibited negligible activity. Reprinted with permission from ref 260. Copyright 2003 American Chemical Society.

ment of electrons and holes is primarily governed by the well-known quantum confinement.300 Generally, a decrease in particle size could be expected to lead to a higher efficiency in photocatalysis.163,916-920 This was because the bulk charge recombination of photogenerated electrons and holes, dominant in the well-crystallized large semiconductor particles, was reduced by decreasing particle size. Reduction in particle size could also lead to a larger surface area and increased the available surface active sites.209,921,922 Lee et al. reported that the smaller particle size and higher surface area of NaTaO3 led to its high photocatalytic activity in overall water splitting.209 They proposed that this was due to the increased probability of surface reactions between the electrons and holes rather than recombination in the bulk. Sathish et al.923 found that CdS nanoparticles showed a higher photocatalytic activity for hydrogen evolution compared to bulk CdS. This was correlated well with the particle size and surface area. Lunawat et al. also found that, compared to bulk CdS, its nanocrystallites dispersed into the channels of mesoporous silicate SBA-15 exhibited enhanced photocatalytic activity for water splitting under visible light.924 This result illustrated the fact that the smaller particle size was capable of enhancing the photocatalytic activity of a semiconducting material. However, the photocatalytic activity does not monotonically increase but even decreases with the decreasing particle size. This is because surface charge recombination can become an important process. When particle size of the nanocrystalline semiconductor becomes extremely small, this in return can offset the benefits of the ultrahigh surface area of the nanocrystalline particles.921,925 Wang et al. showed that there existed an optimal particle size for the pure nanocrystalline TiO2 photocatalyst used in the photocatalytic reaction of chloroform decomposition.926 A similar phenomenon for K2Ta2O6219 and CdS nanocrystals927,928 was also reported. It was found that the optimal particle size was important to achieve the high photocatalytic activity for water splitting. Neither the smallest nor the largest nanocrystals showed the highest photocatalytic activity for


hydrogen evolution. The smallest nanocrystals suffered more from the charge recombination on the surface, whereas, to some extent, the largest nanocrystals suffered from the same disadvantages as large-size particles. Hong et al. investigated the effects of crystal size on photoanode materials based on WO3 in both a particulate suspension (PS) system and a photoelectrochemical (PEC) film system.929 In the PS system, the large crystals showed higher photoactivity because of a well-developed space charge layer and high crystallinity, whereas in the PEC system, the smaller crystals performed better because of the reduced hole diffusion length. These different behaviors were attributed to different chargeseparation mechanisms in the two systems. Bala´zs and coworkers investigated the effect of particle shape on the activity of nanocrystalline TiO2 photocatalysts in phenol decomposition.930-932 They found that the average particle diameter of the best photocatalysts was in the range of 50-70 nm, and the photocatalyst containing only polyhedral nanocrystals displayed better photocatalytic performance than those containing both spherical and polyhedral nanocrystals. Since the first report on the ordered mesoporous silica material MCM-41,933 inorganic materials with controlled porosity have been widely exploited in photocatalysis.934-940 These mesoporous photocatalysts possess two major beneficial characteristics. The first is the high specific surface area, which provides more reactive sites at the surface for photocatalytic reaction to occur. The second is the nanoscale channel wall of mesopores, which can facilitate the transfer of photogenerated electrons and holes to the surface, thus avoiding their recombination in the bulk.80,158,202 For example, different kinds of mesoporous TiO2-based photocatalysts have been previously reported as being promising candidates for efficient charge separation and transport, leading to higher efficiency in photocatalysis for water splitting.80,889,941-946 The mesoporous-assembled SrTiO3 nanocrystal photocatalysts also exhibited much higher photocatalytic activity than the nonmesoporous-assembled commercial SrTiO3 photocatalysts.947,948 Domen and co-workers reported that, although the inorganic phases are amorphous, the photocatalytic activities for overall water decomposition over mesoporous Ta2O5 and Mg-Ta oxide are much higher than over crystallized Ta2O5 and MgTa2O6, respectively.202,204 This high activity was due to the thin walls of the mesopores, which provided a shorter distance for the excited electrons and holes to travel to the surface. Chen et al. found that the photocatalytic activity of mesoporous Nb2O5 was 20 times higher than the bulk, which lacks porosity.158 It was proposed that the positive effect of mesoporosity on the photocatalytic activity was abscribed to the oriented movement and efficient separation of electrons and holes, as shown in Figure 35. The mesoporous In-Nb mixed-oxide catalyst also showed photocatalytic activity for water splitting. This was attributed to the synergistic effects of a high surface area and the well-dispersed indium species intercalated into the mesoporous structure.159 Sang and co-workers synthesized the complex oxide InVO4 with a mesoporous wormhole-like structure.949,950 It had a highly efficient photocatalytic activity due to the low recombination rate of the photoexcited electrons and holes. Ta3N5 with a crystalline mesoporous framework showed the photocatalytic performance for hydrogen evolution greatly superior to that of conventional bulk Ta3N5. The thin-wall structure promoted charge transfer to active surface sites.951 Wang and co-workers suggested that the efficiency of


Chen et al.

Figure 35. Model of photocatalytic H2 evolution on a bulk photocatalyst (a) and a mesoporous photocatalyst (b). Reprinted with permission from ref 158. Copyright 2007 Elsevier.

hydrogen production could be improved by about an order of magnitude through the introduction of mesoporosity into polymeric C3N4.952,953 Bao et al. prepared nanoporous CdS nanostructures using a two-step aqueous route, which displayed very high photocatalytic efficiency for hydrogen production under visible-light irradiation.732 The quantum yield was found to be ∼60.34% at 420 nm. This high activity was due the fact that the fast transport of the photogenerated carriers to the surface of the CdS by traveling only a short distance through the nanopore wall was so advantageous. It greatly decreased the bulk charge recombination, increased the quick surface charge separation and fast interfacial charge carrier transfer, and ensured the fast photochemical reaction at the CdS/electrolyte interface. Feng and co-workers developed a series of porous chalcogenides with openframework construction as efficient photocatalysts for the reduction of water: Na14In17Cu3S35 · xH2O, Cu8Ge5S164-.954-956 It was demonstrated that the open-framework construction helped not only to increase the number of active reaction sites owing to a high surface area but also to reduce the rate of charge recombination of the electron-hole pair. Kudo’s group was the first to report the positive effect of the ordered surface structure on the photocatalytic activity for water splitting. The photocatalytic activity of La-doped NaTaO3 with an ordered surface nanostep structure was 9 times higher than that of nondoped NaTaO3. This was mainly because the ordered surface nanostep structure created by La doping (as shown in Figure 36) contributed to the separation of the photoactive sites in avoiding surface charge recombination and back-reactions.20,216 A similar effect of the surface nanostructure was also observed on some sulfide photocatalysts, such as (AgIn)0.22Zn1.56S2537 and AgGa0.9 In0.1S2544 solid solution. It was proposed that such nanostructured surface edges improved the photocatalytic properties because the incident photon was not shielded and the photogenerated electrons could more easily migrate to the edge of the nanostructured step. Hence, both compounds had enhanced photocatalytic activity for hydrogen evolution under visible-light irradiation. Jing and Guo prepared a highly stable and active CdS photocatalyst through thermal sulfidation of a CdO precursor.957 The special nanostep structure was also observed at the surface of the sulfide photocatalyst, which further supported the premise that the nanostep surface was crucial for the remarkable enhancement of photocatalytic hydrogen production through active sites in suppressing the surface-charge recombination of photogenerated electrons and holes.

Figure 36. Ordered surface nanostep structure of NiO/NaTaO3: La (a), and mechanism of highly efficient photocatalytic water splitting over NiO/NaTaO3:La photocatalysts (b). Reprinted with permission from ref 20. Copyright 2003 American Chemical Society. Ordered surface nanostep structure of Pt/(AgIn)0.22Zn1.56S2 (c) and CdS (d). (c) Reprinted with permission from ref 537. Copyright 2004 American Chemical Society. (d) Reprinted with permission from ref 957. Copyright 2006 American Chemical Society.

Figure 37. Schematic structure of the active NiO-K4Nb6O17 photocatalyst and the reaction mechanism of H2O decomposition into H2 and O2. Reprinted with permission from ref 55. Copyright 2009 The Royal Society of Chemistry.

Some ion-exchangeable layered oxides have been shown to be highly active photocatalysts with several distinct advantages compared to the so-called “bulk” type photocatalysts such as TiO2 or SrTiO3.135,162,164,171,231,958-960 Because of their unique structural characteristics, such layered photocatalysts utilize the intercalated water molecules as reactants to produce hydrogen and oxygen.135,164 K4Nb6O17 has an ion-exchangeable layered structure with two different kinds of alternating interlayer spaces, i.e., interlayers I and II, as shown in Figure 37, which are the active sites for the production of hydrogen and oxygen, respectively.164 It was proposed that the electrostatic gradient in the niobate sheet caused by the different locations of the K+ and H+ cations between interlayer I and II could drive the electrons and holes to move to different active sites, giving rise to efficient charge separation. Domen and co-workers found that a Ni-loaded ion-exchangeable layered oxide K2La2Ti3O10 showed high photocatalytic activity for water splitting.23,135,139 K2La2Ti3O10 had only one type of interlayer space, and most of the loaded Ni existed at the external surface. It was proposed that H2 evolved on the Ni particles at the external surface and O2 evolved in the interlayer space. This again indicated efficient charge separation and suppression of back-reaction were achieved due to the layered structure.



Figure 38. (A) Hydrogen photoproduction in a photoelectrochemical cell consisting of titania nanotube array photoanode and Pt mesh cathode. (inset) FESEM images of titania nanotube arrays. Reprinted with permission from ref 977. Copyright 2005 American Chemical Society. (B) Photoconversion efficiency during water photolysis and maximum photocurrent obtained using TiO2 nanotube-array photoanode as a function of the geometric roughness factor of the nanotube arrays. Reprinted with permission from ref 980. Copyright 2007 IOP Publishing Ltd.

Yoshimura et al. found that different H2 evolution sites in the layered structure led to quite different photocatalytic activities for hydrogen production.959 Pt/HPb2Nb3O10 with Pt in the interlayer space exhibited much higher activity than that with Pt only on the external surface. For the latter case, the electrons had to transfer a long distance through a twodimensional niobate sheet to reduce H+ on the external Pt. There was a short distance for electrons to transfer to the intercalated Pt, and the possibility of charge recombination was largely reduced. They also found that the intercalation of water or hydronium ion into the interlayer space was a key factor in increasing the photocatalytic activity of layered oxides for hydrogen evolution. The intercalation resulted in a dramatic increase in reaction sites for water decomposition along with efficient charge separation.959,961 Moreover, pillared layered photocatalyts showed a marked increase in hydrogen production activities compared with the original layered oxides.98,189 This may be due to the increase of surface area98,962 and/or interlayer spacing,189 which facilitated the reaction between photogenerated charges and reactant molecules and suppressed charge recombination. Various architectures with nanometer- and micrometersized dimensions have been found to play an important role in achieving fast charge transfer and efficient charge separation for the improvement of photocatalytic activity.963 Onedimensional (1D) nanostructures, such as nanowires,730,964,965 nanotubes,99,966-969 and nanorods/nanoribbons,970-974,177 have all displayed great potential in environmental/energy photocatalysis applications. Jitputti and co-workers reported that TiO2 nanowires with high crystallinity and surface area could promote higher H2 evolution than commercial TiO2 nanoparticles.964,975 It was proposed that the unique 1D structure might facilitate the electron transport for reacting with water molecules adsorbed at the TiO2 surface along the 1D structure. Additionally, TiO2 nanofibers prepared by electrospinning techniques showed enhanced crystallinity, surface area, and photocatalytic activity for hydrogen evolution compared to nanofibers prepared by hydrothermal method.975 Li and Lu demostrated that one apparent advantage of Na2Ti2O4(OH)2 nanotubes for photocatalytic hydrogen production over TiO2 particles was their one-dimensional tubular structure, which was favorable for electron transfer and thus reduced the recombination of electron-hole pairs.649 Grimes and co-workers examined the use of titania nanotube arrays for the photocleavage of water into hydrogen and oxygen under UV irradiation.976-982 The nanotubular

architecture gave rise to superior electron lifetimes and, hence, more efficient charge separation.977,983 On a per-watt basis, the hydrogen generation rate obtained of 24 mL/(h W) was among the highest reported for a titania-based photoelectrochemical cell, as shown in Figure 38A.977 They also claimed that TiO2 nanotube-array photoanodes could generate H2 by water photolysis with a photoconversion efficiency of 16.5% under UV light illumination (Figure 38B).980 A three-step electrochemical anodization was demonstrated to contribute to the formation of highly ordered TiO2 nanotube arrays and then greatly enhance the photoelectrochemical and hydrogen evolution activities.984 Cho et al. found that single-crystalline SrNb2O6 nanotubes with rhombic cross sections exhibited superior photocatalytic activity for the H2 evolution from pure water compared to their bulk counterparts.985 This was attributed to the higher surface area and the smaller diffusion length of the charge carriers resulting from the morphological characteristics of the material. It was reported that the photocatalytic activity enhancement of TiO2 nanorods could be attributed to the larger surface area,970,973 which promoted the probability of a surface reaction between the electrons and holes rather than recombination in the bulk.209 Chen and Ye found that, under UV irradiation, nanorod-like SrSnO3 had a photoactivity 10 times greater than the particles prepared by a solid-state reaction.268 Porous nanorod-structured ZnFe2O4 showed effective H2 evolution from methanol aqueous solution under visible light. The nanorod shapes and their intraparticle porous structures were proven to be beneficial for more quickly transferring the photogenerated carriers onto the surfaces, which in return favored the efficient charge separation.986 The high electron mobility in 1D nanostructured nanorods also partially contributed to the high photocatalytic hydrogen yield of the (Cd0.8Zn0.2)S nanorods.987 A device physics model for radial p-n junction nanorod solar cells was developed by Kayes et al.988 Densely packed nanorods were oriented with the rod axis parallel to the incident light direction. The study indicated that high-aspectratio (length/diameter) nanorods allowed the use of a sufficient thickness of material to obtain good optical absorption while simultaneously providing short collection lengths for excited carriers in a direction normal to the light absorption. The design of the radial p-n junction nanorod device could provide large improvements in efficiency relative to a conventional planar geometry.


Chen et al.

electrons transfer from the nanosheets with high electricpotential to the core micropyramid with low electricpotential. The probability of photogenerated electron/hole pair recombination was thus reduced. Kale et al. reported that CdIn2S4 nanostructures with a marigold-like morphology composed of numerous nanosized petals displayed high photocatalytic activity for solar production of hydrogen from H2S in KOH aqueous solution.1010

6. Photocatalytic Hydrogen Generation Systems

Figure 39. Model of the movements of the photoproduced electron and hole at the TiOx nanosheet with a lepidocrosite-type structure. The electron moves in the 3d CB consisting of the Ti4+ network in the nanosheet and then reduces Ag+ and Cu2+ at the edge, whereas the hole exists at the 2p VB consisting of the O2- surface and oxidizes Mn2+ on the surface. Reprinted with permission from ref 993. Copyright 2008 American Chemical Society.

Two-dimensional (2D) nanostructures such as nanobelts,989-991 nanosheets,992-994 and nanoplates995,996 also favor the transfer of electrons and holes generated inside the crystal to the surface and promote the charge separation, which helps to enhance the photocatalytic activity to some degree.991,997-1001 Sun et al. found that the photocatalytic properties of ZnO nanobelt arrays was better than that found for ZnO film or the rod-/comblike ZnO nanostructures under identical conditions.989 Ultrathin nanosheets of brookite TiO2 displayed high phtocatalytic activity. The atomic scale thickness and large surface area allowed shorter migration time of carriers, suppressed bulk recombination and more electrons and holes on the surface.1002 Jitputti et al. reported that nanosheet TiO2 exhibited higher photocatalytic activity for hydrogen evolution than that of commercial TiO2 anatase powder.1003 Matsumoto et al. observed the separate photocatalytic active sites on the TiOx nanosheets by photodepositing metal and metal oxide.993 As shown in Figure 39, the photogenerated electrons mainly reacted at the edge of the nanosheets, whereas the photogenerated holes reacted all over the surface. Thus, the recombination of electrons and holes in the TiOx nanosheets was to some extent impeded. Osterloh and coworkers developed a modular approach to the synthesis of nanostructured catalysts for photochemical water-splitting catalysts based on exfoliated, semiconducting niobate nanosheets.188,1004-1007 These could be integrated into twocomponent nanostructures with separate sites for water reduction and oxidation. Zhang and Zhu revealed that Bi2WO6 nanoplates had a special advantage in photocatalytic reactions, because the nanoplate structure not only had a larger surface area but also promoted the efficiency of the electron-hole separation.996 Self-assembly of nanoscale building blocks into threedimensional (3D) complex structures is another research hot spot in photocatalysis.1008-1013 Song and Gao found that hollow NiO microspheres showed a significantly more enhanced photocatalytic activity than NiO rods.1008 The increasing number of surface active sites and surface charge carrier transfer rate in the photocatalysis of the hollow NiO microspheres proved advantageous. Lu et al. reported that quite a good photocatalytic performance was obtained on a novel ZnO hierarchical micro/nanoarchitecture with dense nanosheet-built networks standing on hexagonal-pyramidlike microcrystals.1009 This was because the special structural features of the micro/nanoarchitectured ZnO promoted

The tremendous effort put into the synthesis and modification of photocatalysts to adjust their band structures and increase the probabilty of photogenerated charge separation has resulted in the progressive development of highefficiency visible-light-driven photocatalysts. Meanwhile, it is widely believed that the construction of appropriate and efficient photocatalytic hydrogen generation systems (solution/semiconductor suspensions) based on different kinds of photocatalysts is an indispensable step to achieving high performance for photocatalytic hydrogen generation.

6.1. Hydrogen Generation Systems Containing Sacrificial Reagents The basic principle of photocatalytic reactions for hydrogen/ oxygen generation using electron donors/acceptors as the sacrificial reagents is depicted schematically in Figure 40.51 When the system is constructed in the presence of an electron donor, the photogenerated holes irreversibly oxidize the reducing electron donors instead of H2O. If the bottom of the conduction band of the photocatalyst is located at a more negative potential than the water reduction potential, this then facilitates water reduction by the photogenerated electrons in the conduction band.51,300 The different kinds of typical sacrificial reagents are shown in Table 3.

6.1.1. Inorganic Sacrificial Reagent Systems 6.1.1.1. S2-/SO32- System. Since S2- and SO32- could be oxidized by photogenerated holes to Sn2- and SO42-, respectively, they can thus act independently as sacrificial reagents for photocatalytic hydrogen generation.848,849,1014-1017 However, the oxidation of S2- ions to yellow polysulfides Sn2- leads to a decrease in H2 formation over time. This is due to the high light absorption of the yellow polysulfide Sn2- in the visible region and then to the competitive reduction of Sn2- with H2O.1014,1018-1020 Fortunately, SO32could act as Sn2--regenerating agent and maintain the solution colorless.1021 Therefore, the S2-/SO32- mixture is most widely used as electron donors and added to the water/semiconductor suspension to improve the photocatalytic activity and stability

Figure 40. Basic principle of photocatalytic reactions in the presence of sacrificial reagents. Reprinted with permission from ref 51. Copyright 2007 American Chemical Society.

mass (g) 0.3 0.2 0.2 0.25 0.025 0.1 1 0.1 1 0.1 0.2 1 0.3 0.2 0.08 0.08 0.01 0.1 0.1 0.08 0.02 0.1 0.05 0.005 0.05 0.05 0.02 0.1 0.1 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.08 0.08 0.08 0.04 0.04 0.04 0.02 0.01 0.16 0.16 0.3

photocatalyst

Pt-PdS/CdS Pt/WS2/TiO2 Pt/CdS/Ti-MCM-41 ZnFe2O4/SrTiO3 Pt-PdS/CdS MoS2/CdS RuO2/K2La2Ti3O10:Zn Pt/TiO2 KBi3PbTi5O16 Pt/SrTiO3:Rh NiO/TiO2 Pt/H2LaNb2O7:In Pt-Ru/Y2Ta2O5N2 NiOx/CdS/KNbO3 Pt/TiO2 Pt/TiO2 Pt/Cu2O Pt/TiO2 Ni-La2O2CO3 Pt/TiO2 DPt/TiO2 Pt/TiO2:Gd Wells-Dawson heteropoly blue/Pt/TiO2 H4Nb6O17/Pt/Ru(bpy)2(4,4′-(PO3H2)2bpy)2+ Pd/TiO2 Pt/TiO2:B,N TiO2/Rh/Eosin-Y TiO2/Pt/Fe3+-Eosin-Y MoS2/CdS Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 WOx/TiO2 WOx/TiO2 Pt/TiO2

2-

S /SO3 S2SO32S2O32H2S lactic acid IBrCe3+ Fe2+ CNmethanol ethanol isopropanol 1-propanol 1-butanol formic acid acetic acid formaldehyde acetaldehyde oxalic acid glycol glycerol EDTA glucose sucrose diethanolamine TEA lactic acid n-pentane n-heptane isooctane n-paraffin polyethylene benzene phenol pyridine coal tar sand pitch Acid Orange 7 Basic Red 46 Basic Blue 41 monochloroacetic acid dichloroacetic acid trichloroacetic acid monoethanolamine hydrazine dihydrochloride 2,4-dichlorophenoxyacetic acid 4-chlorophenol Polyvinyl alcohol

2-

sacrificial reagent

Table 3. Typical Sacrificial Reagent Contained Photocatalytic Hydrogen Production System

300-W Xe (>420 nm) 350-W Xe (>430 nm) 350-W Xe (>430 nm) 600-W W 300-W Xe (>420 nm) 300-W Xe (>420 nm) 250-W Xe 500-W Hg 450-W Hg 300-W Xe (>420 nm) 450-W Hg 100-W Hg (>290 nm) 300-W Xe (>420 nm) 500-W Hg-Xe (>400 nm) 500-W Xe 500-W Xe H (>420 nm) 300-W Hg 125-W Xe (>400 nm) 500-W Xe 250-W Hg 1200-W Ultra-Vitalux 300-W H (>420 nm) 300-W Xe (>420 nm) 125-W Hg 300-W Xe 200-W H (>420 nm) 400-W H (>420 nm) 300-W Xe (>420 nm) 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 250-W Hg 250-W Hg 250-W Hg 200-W Hg 500-W Hg 250-W Naa 250-W Na 500-W Xe

light Source 29 233 890 76 410 688 ∼94 000 ∼5300 55.5 ∼550 35.21 169 1500 5268 833 203.5 ∼150 ∼75 155 28 380 36 45.3 2800 13 775 ∼62.5 4320 4580 ∼2500 1185.5 2750 5400 28 36.7 31.3 7.7 13 120 110 103.3 30 33.3 33.3 ∼502.5 ∼187.5 ∼112.5 375 197 trace 191.7 ∼8370 ∼0.036 ∼0.005 28.7

rate of hydrogen evolution (µmol · h-1 · g-1)

∼0.66 (380 nm)

10.27 (>420 nm) 19.1 (>420 nm)

20.0 (670 nm) 22 (450 nm)

8.8 (>400 nm)

0.32 1.54 (>290 nm)

30 (420 nm)

2.6 (420 nm)

93 (420 nm)

quantum yield (%)

733 850 849 872 785 782 140 1051 146 1046 1052 183 393 800, 801 1066 1066 1075 1064 1065 1066 1056 82 637, 638 623, 624 1085 455 647 654 782 1070 1070 1070 1070 1070 1070 1070 1070 1070 1070 1070 1071 1071 1071 1073 1073 1073 1074 1076 1082 1082 1083

reference


for hydrogen evolution from water.732,733,1022-1027 For example, a quamtum yield of ∼93% at 420 nm has recently been reported for the Pt-PdS/CdS photocatalyst, the highest photocatalytic activity so far achieved for hydrogen production in the presence of sacrificial reagents of S2-/SO32- under visible-light irradiation.733 The reaction mechanism in the presence of S2-/SO32- as sacrificial reagent is described by eqs 6-11.732

∼0.3 (380 nm) ∼1.7 (380 nm) ∼0.97 (380 nm) ∼1 (380 nm) ∼0.55 (380 nm) ∼0.68 (380 nm) ∼0.25 (380 nm) ∼2.1 (380 nm) ∼2.6 (380 nm) ∼1.35 (380 nm) ∼0.75 (380 nm) ∼0.66 (380 nm) ∼1.43 (380 nm) ∼1.52 (380 nm)

1083 1083 1083 1083 1083 1083 1085 1083 1083 1083 1083 1083 1083 1083 1083 1083 1083 1083 1083 1083 1083 ∼0.35 (380 nm) ∼0.027 (380 nm) ∼0.37 (380 nm) ∼0.42 (380 nm) ∼7 (380 nm) ∼1.8 (380 nm)

photocatalyst + hυ f h+ + e-

(6)

2e- + 2H2O f H2 + 2OH-

(7)

SO32- + 2OH- + 2h+ f SO42- + 2H+

(8)

2S2- + 2h+ f S22-

(9)

S22- + SO32- f S2O32- + S2-

(10)

SO32- + S2- + 2h+ f S2O32-

(11)

Sodium lamp.

Since S2O32- could be oxidized to SO32- and subsequently to SO42- by photogenerated holes, it has also been occasionally used as a sacrificial reagent for photocatalytic hydrogen generation.870,871,1028-1030 6.1.1.2. H2S-Splitting System. A particularly meaningful system from the point of view of energy conservation and environmental protection is the photocatalytic hydrogen generation from H2S dissolved in water or alkali solution.398,785,806,1010,1031-1041 This approach via H2S could have practical applications using waste gas H2S from chemical industries such as natural gas utilization and desulfurization process in petrochemical plants.56,1042 When H2S is dissolved in alkaline aqueous solution, sulfide ions are formed and henceforth can play the role of sacrificial reagent. As described by eqs 6 and 12-14, the overall process corresponds to H2S splitting by two photons of visible light. This requires 39.3 kJ/mol.1043,1044

a

quantum yield (%)

500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 125-W Hg 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 500-W Xe 0.3 0.3 0.3 0.3 0.3 0.3 0.05 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 0.3 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2 Pt/TiO2

polyvinylchloride Teflon trichlorobenzene trichloroethylene sugar starch microwave treated soluble starch cellulose (filter paper) glycine glutamic acid proline gelatin stearic acid olive oil Chlorella Laver rice plant turf cockroach human (urine, feces) cow dung

rate of hydrogen evolution (µmol · h-1 · g-1) light Source sacrificial reagent mass (g) photocatalyst

Table 3. Continued

Chen et al.

15 1.17 16 18.3 306.7 80 ∼1857 13.3 73.3 42 43.3 23.7 29.3 10.7 90 110.7 58.3 32.7 28.7 58.7 66

reference


H2S + OH- f HS- + H2O

(12)

2HS- + 2h+ f S22- + 2H+

(13)

2H+ + 2e- f H2

(14)

Recently, Li and co-workers developed a nonaqueous ethanolamine solution as the solvent and reaction medium for the direct splitting of H2S into H2 and S on a CdS-based photocatalyst under visible-light irradiation.785 The potential of H2S splitting in ethanolamine was greatly lowered, and the photogenerated electrons could be fully used to reduce protons for hydrogen production. The quantum efficiency was as high as 30% under visible-light irradiation. They also investigated hydrogen generation using gas-solid-phase photocatalytic H2S splitting on semiconductor photocatalysts.1045 However, performance under gas-solid-phase conditions was substantially lower than that under liquidsolid-phase conditions. 6.1.1.3. Other Inorganic Sacrificial Reagent Systems. Other inorganic ions, such as Fe2+,274,752,1046,1047 Ce3+,146,1048,1049 I-,140,351,613,625,626,642-644,1050 Br-,1051 and CN-,1052 have also been used as sacrificial reagents for hydrogen generation. These inorganic ions were easily oxidized by the photoge-



nerated holes to Fe3+, Ce4+, I3- (or IO3-), Br2, and OCN-, respectively. The result is hydrogen generation via water reduction by photogenerated electrons. Taking I- as an example of an inorganic sacrificial reagent, the photocatalytic mechanism for hydrogen generation is described as eq 6 and eqs 15 and 16.1050

photocatalytic H2 generation from fossil fuels and hydrocarbons with water with powdered Pt/TiO2 catalyst suspended in solution.1070 The mechanism for photocatalytic H2 generation from aqueous solutions of hydrocarbons could be explained by eq 6 and eqs 24-30.1070

2H+ + 2e- f H2

H2O + h+ f ·OH + H+

(24)

H+ + e- f 1/2H2

(25)

{

(15)

3I- + 2h+ f I3- (in acidic solution)

I- + 6OH- + 6h+ f IO3- + 3H2O (in basic solution)

}

(16)

Some photooxided species, such as Fe3+, Ce4+, and IO3-, could be easily reduced by photogenerated electrons back to Fe2+,269,336,764,1053 Ce3+,269,1049 and I-,1054 respectively. Thus, they could act as electron acceptors for photocatalytic oxygen generation from aqueous solution. Fe2+/Fe3+, Ce3+/Ce4+, and I-/IO3- have therefore been used as redox mediators to construct a suitable system for overall water splitting using the Z-scheme system shown in section 6.2.2.

6.1.2. Organic Sacrificial Reagent System Organic compounds, such as alcohols (methanol, ethanol, isopropanol, etc.),82,91,1054-1061 organic acids (formic acid, acetic acid, etc.),91,938,1062-1064 and aldehydes (formaldehyde, acetaldehyde, etc.)91,1056,1065,1066 have all been used as electron donors for photocatalytic hydrogen generation. Among them, methanol was most widely used, and the hydrogen generation process is described as eq 6 and eqs 17-21:183,184,1067

h+ + H2O f ·OH + H+

(17)

CH3OH + ·OH f ·CH2OH + H2O

(18)

+

-

·CH2OH f HCHO + H + e

(19)

2H2O + 2e- f H2 + 2OH-

(20)

hυ,catalyst

overall reaction: CH3OH 98 HCHO + H2 (21) The product, formaldehyde (HCHO), could be further oxidized to methanoic acid HCOOH and subsequently to CO2 together with hydrogen generation via eqs 22 and 23:1054,1068,1069 hυ,catalyst

HCHO + H2O 98 HCOOH + H2

(22)

hυ,catalyst

HCOOH 98 CO2 + H2

(23)

In these photocatalytic systems, organic compounds are oxidized and decomposed by the photogenerated holes. Meanwhile, the remaining photogenerated electrons reduce water to hydrogen. Thus, it can be envisaged that a bifunctional photocatalytic system could be constructed, in which organic pollutants will be used to act as electron donors that achieve photocatalytic production of hydrogen from polluted water and simultaneous degradation of organic pollutants.91,1066 Hashimoto et al. pioneered the work on

RCH2CH3 + 2·OH f RCH2CH2OH + H2O (26)

RCH2CH2OH f RCH2CHO + H2

(27)

RCH2CHO + H2O f RCH2COOH + H2

(28)

photo-Kolbe reaction: RCH2COOH f RCH3 + CO2 (29)

hυ, catalyst

overall reaction: RCH2CH3 + 2H2O 98 RCH3 + 3H2 + CO2 (30) To date, different kinds of model pollutants (azo-dyes, oxalic acid, formic acid, formaldehyde, chloroacetic acids, acetic acid, EDTA, dithiothreitol, TEA, hydrazine, dichlorophenoxyacetic acid, chlorophenol, etc.) were used as electron donors to construct the bifunctional photocatalytic systems. The photocatalytic decomposition of organic pollutants happened synchronously with efficient hydrogen generation.649,1056,1064,1071-1082 Furthermore, it has been suggested that the photocatalytic reforming of biomass, which serves as the energy resource in plants and animals, may be anthor promising way of producing hydrogen from water. Kawai and Sakata constructed a water splitting system based on TiO2 catalyst for photocatalytic hydrogen production involving decomposition of protein, algae, dead insects, and excrement with CO2 as the only byproduct.1083,1084 Carbohydrates, such as starch, cellulose, glycerol, glucose, and sucrose, were used as the sacrificial electron donors to construct water-splitting system for hydrogen generation by photocatalytic reforming of biomass over metal-loaded TiO2 catalysts as well.455,755,1084-1089 A probable mechanism for the photocatalytic reforming of glucose for hydrogen generation over Pt/TiO2 was proposed by Fu et al.1085 The reactions involved in the mechanism are summarized by eqs 31-37 and Figure 41.

Pt/TiO2 + hυ f e- + h+

(31)


Chen et al.

Figure 41. Proposed mechanism of the photocatalytic reforming of glucose on Pt/TiO2. Reprinted with permission from ref 1085. Copyright 2008 Elsevier.

{

h+ + H2O f H+ + ·OH

(32)

H+ + e- f 1/2H2

(33)

(RCH2OHdC6H12O6) + RCH2OH f H+ + RCH2O-

{

H+ + e- f 1/2H2 -

+

RCH2O + h f RCH2O· ˙ HOH + RCH2OH RCH2O· + R′CH2OH f R′C

}

(34)

˙ H2OH + h+ f H+ + R′C˙HO· f R′CHO R′C H+ + e- f 1/2H2

(35) R′CHO + ·OH f [R′COOH]- + H+ H+ + e- f 1/2H2 -

(36)

+

[R′COOH] + h f R′H + CO2 hυ,catalyst

overall reaction: C6H12O6 + 6H2O 98 6CO2 + 12H2 (37) In spite of the limited work in this special area, the results are encouraging and promising for the construction of photocatalytic systems involving efficient hydrogen generation as well as pollutant decomposition or biomass reforming.

6.2. Overall Water-Splitting Systems 6.2.1. Pure Water-Splitting System As illustrated in Figure 3, the photocatalyst acts as two roles, H2 generators and O2 generators in the overall pure water-splitting system. Over the past several decades, a number of photocatalysts have been successfully developed to construct an overall water-splitting system for simultaneous hydrogen and oxygen generation in the absence of sacrificial reagents.20,22,24,51,353,1090 Among them, (Ga1-xZnx)(N1-xOx) has been proven as the most promising

photocatalyst for overall water splitting.575 Steady and stoichiometric H2 and O2 evolutions were found to evolve with a quantum yield of 5.9% in the range of 420-440 nm.575

6.2.2. Biomimetic Z-Scheme Water-Splitting System The biomimetic Z-schem system mechanism using reversible redox mediators has been investigated with a view to constructing a photocatalytic system for overall water splitting into H2 and O2. For example, Arakawa and co-workers constructed an artificial Z-scheme system for overall water splitting using WO3 photocatalyst and a Fe2+/Fe3+ redox mediator.1091,1092 Kozlova et al. investigated the overall water splitting over a Pt/TiO2 catalyst with a Ce3+/Ce4+ shuttle charge transfer system.1048 However, in these studies, the photocatalytic activities for O2 and H2 production were low, due to the back-reaction and the interactional reaction characteristics. Fujihara et al. constructed a Z-scheme watersplitting system using a TiO2-rutile photocatalyst and two redox mediators (Br2/Br- and Fe3+/Fe2+) in a two-compartment cell.1051 As the production of H2 and O2 were carried out in separated compartments, the reversible reactions on photocatalysts, which often suffered from the effects of backreactions, were largely prevented. Abe et al. used an innovatively designed Z-scheme system for overall water splitting into H2 and O2 using a two-step photoexcitation.1093 It was composed of an IO3-/I- shuttle redox mediator and two different photocatalysts: Pt-loaded anatase TiO2 for H2 evolution and rutile TiO2 for O2 evolution. The proposed photocatalytic reaction mechanism for the Z-scheme water-splitting system is depicted schematically in Figure 42. Under UV irradiation, simultaneous gas evolution of H2 (180 µmol/h) and O2 (90 µmol/h) was observed from a basic (pH ) 11) NaI aqueous suspension of these two different TiO2 photocatalysts. The overall water splitting proceeded by the redox cycle between IO3- and Iunder basic conditions as follows: (a) water reduction to H2 and I- oxidation to IO3- over Pt-TiO2-anatase and (b) IO3reduction to I- and water oxidation to O2 over TiO2-rutile. IO3- reduction to I- over Pt-TiO2-anatase was an undesirable side reaction. If this reaction was suppressed, the total water-splitting reaction took place more efficiently. The



Figure 42. Proposed photocatalytic reaction mechanism for Z-scheme water-splitting system using an IO3-/I- redox mediator and a mixture of Pt-TiO2-antase and TiO2-rutile photocatalysts. Reprinted with permission from ref 1093. Copyright 2001 Elsevier.

advantage of this system was that H2 gas was evolved only over the Pt-TiO2-anatase photocatalyst and that O2 gas was evolved over the TiO2-rutile photocatalyst only, even from a mixture of IO3- and I- in a basic aqueous solution. Therefore, another undesirable backward reaction, H2O formation from H2 and O2 on Pt particles, was suppressed.1093 In the later studies, a series of Z-scheme overall watersplitting systems active under visible-light irradiation were constructed, such as (Pt/ATaO2N (A ) Ca, Sr, Ba))-(Pt/ WO3)-(IO3-/I-),395,1094 (Pt/TaON)-(Pt/WO3)-(IO3-/I-),471 (Pt/SrTiO3:Cr/Ta)-(Pt/WO3)-(IO3-/I-),345,1095,1096 (Pt/ZrO2TaON)-(Pt/WO3)-(IO3-/I-),897,1097 (Pt/TaON)-(RuO2/ TaON)-(IO3-/I-),1098 (Ru/SrTiO3:Rh)-(BiVO4)-(Fe3+/ Fe2+),752 (Pt/SrTiO3:Rh)-(Bi2MoO6)-(Fe3+/Fe2+),1046 (Pt/ SrTiO3:Rh)-(WO3)-(Fe3+/Fe2+),1046,1047 (Pt/SrTiO3: Rh)-(BiVO4)-(Fe3+/Fe2+),1046 (Pt/ZrO2-TaON)-(Ir/ Ta3N5-TiO2)-(IO3-/I-),1099 and (coumarin-dye-adsorbed Pt/ H4Nb6O17)-(IrO2-Pt/WO3)-(IO3-/I-).1100 These are summarized in Table 4. Of these, the (Pt/ZrO2-TaON)-(Pt/ WO3)-(IO3-/I-) system showed the highest photocatalytic activity for overall water splitting with a quantum efficiency of ca. 6.3% at 420.5 nm. In this Z-scheme overall watersplitting system, the H2 and IO3- production proceeded over the Pt/ZrO2-TaON photocatalyst; meanwhile, the IO3reduction and water oxidation to O2 took place over Pt-WO3 under visible-light irradiation.1097 In general, a redox mediator (such as IO3-/I- and Fe3+/Fe2+) is required for the construction of a Z-scheme photocatalytic system. Undesirable side effects such as backward reactions to form water from the H2 and O2 evolved can occur. Recently, Kudo et al. had a surprising success in fabricating an overall water-splitting system driven by a Z-scheme interparticle electron transfer between H2- and O2-photocatalysts (Ru/SrTiO3:Rh-BiVO4) without a redox media-

Figure 43. Mechanism of water splitting using the Z-scheme photocatalysis system driven by electron transfer between H2- and O2-photocatalysts. (a) Suspension of Ru/SrTiO3:Rh and BiVO4 at neutral and acidic conditions. (b) Scheme of photocatalytic water splitting. Reprinted with permission from ref 1101. Copyright 2009 American Chemical Society.

tor.1101 This is shown in Figure 43, in which the undesirable reactions and negative effects by an electron mediator were excluded. Although the activity of a Z-scheme overall watersplitting system is quite low and only a little higher than that achieved by conventional pure water-splitting systems using one single photocatalyst, these results provided a promising approach to constructing efficient overall watersplitting systems.

7. Summary and Prospects So far, the sacrificial reagent-containing water-splitting systems constructed based on the Pt/CdS,732 Pt-PdS/CdS,733 and Zn/Cr layered double hydroxide667 photocatalysts demonstrated the best performance for hydrogen production and oxygen production, with the highest quantum yields of ca. 60.35%, 93%, and 60.1%, respectively, at 420 nm. However, the efficiency of an overall water-splitting system based on visible-light-driven photocatalysts has been still quite low, with the maximum quantum efficiency of ca. 5.9% over Rh2-yCryO3/GaN-ZnO in the range of 420-440 nm.575 This is still far from the quantum efficiency (ca. 30% at 600 nm) designated the initial starting point for practical applications51,56

Table 4. Z-Schematic Photocatalytic System for Water Splitting to Hydrogen and Oxygen under Visible-Light Irradiation activity (µmol · h-1 · g-1) H2 photocatalyst

O2 photocatalyst

mediator light source incident light

Pt/TaON (0.2 g) Pt/CaTaO2N (0.1 g) Pt/BaTaO2N (0.1 g) Pt/SrTiO3:Cr/Ta (0.2 g)

Pt/WO3 (0.2 g) Pt/WO3 (0.1 g) Pt/WO3 (0.1 g) Pt/WO3 (0.325 g)

IO3-/IIO3-/IIO3-/IIO3-/I-

Pt/ZrO2-TaON (0.025 g) Pt/TaON (0.05 g) Ru/SrTiO3:Rh (0.05 g) Pt/SrTiO3:Rh (0.02 g) Pt/SrTiO3:Rh (0.02 g) Pt/SrTiO3:Rh (0.02 g) Pt/ZrO2-TaON (0.05 g) coumarin/Pt/H4Nb6O17 (0.05 g) Ru/SrTiO3:Rh

Pt/WO3 (0.05 g) RuO2/TaON (0.05 g) BiVO4 (0.05 g) Bi2MoO6 (0.02 g) WO3 (0.02 g) BiVO4 (0.02 g) Ir/TiO2/Ta3N5 (0.05 g) IrO2-Pt/WO3 (0.1 g) BiVO4

IO3-/IIO3-/IFe3+/Fe2+ Fe3+/Fe2+ Fe3+/Fe2+ Fe3+/Fe2+ IO3-/IIO3-/I-

300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe 300-W Xe

H2

O2

>420 nm >420 nm >420 nm >420 nm

120 43 67 80

60 21 33 24.6

>420 nm >420 nm >420 nm >420 nm >420 nm >420 nm >400 nm >400 nm >400 nm

1040 60 378 950 390 750 ∼45 48.3 400

266 30 179 445 200 360 ∼22 12.1 190

QY 0.4 (420 nm)

ref

471 395 0.1 (420-440 nm) 395 1 (420 nm) 345, 1095, 1096 6.3 (420.5 nm) 897, 1097 0.1-0.2 1098 0.3 (420 nm) 752 0.2 (440 nm) 1046 0.2 (440 nm) 1046 0.3 (440 nm) 1046 1099

Semiconductor-based Photocatalytic Hydrogen Generation - American

Recommend Documents